In the process of trying to calibrate a number of hygrometers, with Sensirion MEMS electronic sensors, I came across the method of using wet salt: an airtight container will stabilize at a predictable relative humidity over time, given a particular salt and temperature.

For a list of salts and their RH values at particular temperatures see this page on the website of Vernier, a maker of STEM education equipment. The various salts suggested for this method repeatably produce a range of low to high relative humidities, also allowing for two-point calibration.

I require my hygrometers be calibrated close to 40% RH. With a predictable 43% RH that makes potassium carbonate the ideal candidate. However, when I wettened potassium carbonate with water it underwent an moderate exothermic reaction. Googling what was going on, I read "potassium carbonate dissociates completely in water into potassium (K+) and carbonate ions (CO32-)."

Which makes me wonder:

Can potassium carbonate be used at all for the wet salt calibration method, or does its swift dissociation render it useless for this application?

  • 2
    $\begingroup$ While there are guides available suitable for checking this at home (example), the question does not mention if the device is electronic, or mechanic. The later will take more time to settle, than the former. In addition if mechanic be aware the ones with natural hair (non-linear scale, especially in the lower values) differ from those based on a synthetic fiber (almost linear scale). Don't forget the natural hair hygrometers need recurrent exposure to high humidity (e.g., bath with shower, not a sauna) to work reliably. $\endgroup$ – Buttonwood Mar 11 at 16:56
  • 1
    $\begingroup$ Updated the original post: the sensors are electronic. $\endgroup$ – user345360 Mar 11 at 17:28
  • 3
    $\begingroup$ @Buttonwood Czechoslovak civil and military stations – I served as military airfield meteorologist, being enlisted in 1989-90 – used in late 80s early 90s as the humidity sensor a mechanically primed animal-origin membrane. It had reportedly much more linear response, compared to hairs. Hair sensitivity is highly nonlinear and dramatically decreases toward 100%. $\endgroup$ – Poutnik Mar 12 at 6:50

Note that all salts, used in humidity calibration, dissociate to their respective hydrated cations and anions when dissolved.

From the solution crystallizes the sesquihydrate $\ce{K2CO3·​\frac 32 H2O}$ ("potash hydrate"). Heating this solid above 200 °C gives the anhydrous salt (Wikipedia).

It seems you have anhydrous carbonate, that hydrates itself exothermically. You can still use it, but you need to prepare rather the saturated solution with excess of carbonate, that would integrate the crystal water into itself.

Or, let the prepared saturated solution partially evaporate and crystalize.

What is important is maintained equilibrium.

$\text{Air 43% humidity }\ce{ <=> K2CO3} \text{ saturated solution } \ce{<=> K2CO3 . 3/2 H2O}$

Anhydrous $\ce{K2CO3}$, wetted by water, rather just absorbs water into its crystall lattice. If you add too little water, no solution would left, similarly what would happen to the plaster of Paris.

You need the carbonate in hydrate form, together with its saturated solution. Take some water, add there carbonate to dissolve as much of as it can, and then some. Let is settle.

If you had the hydrate, you could just moisten it. But you do not have it.

There is the third option - moistening it enough so some liquid phase always remains. For $\pu{100 g }\ce{K2CO3}$, you need about $\ce{20 mL}$ of water just for the crystal water, so it becomes the part of the solid.

The carbonate solubility is $\pu{110.3 g/100 mL}$, so I would carefully mix some $$\pu{100 g}\ \ce{K2CO3} + \pu{50 mL}\ \ce{H2O}$$

or recalculated to more suitable amounts.

  • $\begingroup$ The preparation should become viable naturally, if left exposed to air until the water partially evaporates? $\endgroup$ – user345360 Mar 11 at 13:35
  • $\begingroup$ I do not have the scientific framework to understand your answer. Do you mean the salts should be moistened, not dissolved? $\endgroup$ – user345360 Mar 11 at 17:35
  • 1
    $\begingroup$ See the answer update. $\endgroup$ – Poutnik Mar 11 at 21:32

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service, privacy policy and cookie policy

Not the answer you're looking for? Browse other questions tagged or ask your own question.