A friend asked me to help test a hobby-quality $\ce{CO2}$ sensor MG-811 (updated link). It uses a solid electrolyte and should provide a sensitivity of something like -40 mV per decade. I though I'd just use a small amount of acetic acid + baking soda to make roughly 4,000 ppm in a large container, and compare to "fresh air" which should be roughly 400 ppm, or at least within the 350 to 600 ppm range, as a very rough initial test.

But then I noticed/remembered (duh!) that the acid smells quite strong. Are these simply molecules of $\ce{CH3COOH}$ that are evaporating, or are they bringing along molecules of water in some kind of cluster?

I realized that they could potentially contaminate the sensor, so I'd like to know what I'm up against in terms of removing them from the gas before immersing the sensor.

I've tried to look up the vapor pressure of acetic acid, and it seems to be quite large, about 10 Torr at 20C. See for example here and here. So I'm thinking of using some kind of ad-hoc cold-trap to try to remove it. Might there be another way to do this without using special laboratory equipment? Would passing the gas over dry $\ce{NaHCO3}$ or a solution of it help to "getter" the remaining acetic acid vapor?

Or, is there a better way to produce a controlled amount of $\ce{CO2}$ to begin with?

enter image description here

  • $\begingroup$ A cold trap would be better than trying to pass the gas stream through more baking soda and potentially altering the concentration of the stream to be measured by an unknown amount. Some more details on the proposed test and setup would be helpful. $\endgroup$
    – J. Ari
    Jan 30, 2018 at 1:36
  • $\begingroup$ @J.Ari Thanks, I wasn't aware that gaseous CO2 would react with baking soda in any significant way. $\endgroup$
    – uhoh
    Jan 30, 2018 at 3:08
  • 1
    $\begingroup$ But the remaining acetic acid would unless you make sure that the acetic acid is the limiting reagent to make your CO2. The odor will dissipate in time if the acetic acid is reacted away. $\endgroup$
    – J. Ari
    Jan 30, 2018 at 13:55
  • $\begingroup$ @J.Ari oh for sure. I think you are right, the acid should be the limiting reagent. (I recently learned about limiting reagents a few weeks ago). $\endgroup$
    – uhoh
    Jan 30, 2018 at 15:52

1 Answer 1


You could use a less volatile acid, like oxalic. But I think the reaction with NaHCO3 probably gives off a mist as the reaction bubbles, and that might be why the odor is so strong.

How about using seltzer water (or Perrier? or Diet Coke!) as the source of CO2? I estimate that the pressure of CO2 is about 45 psi in the unopened bottle, and if you attach a balloon to a freshly opened bottle and let it outgas slowly, the balloon will fill up and be essentially pure CO2. If a latex balloon is unsuitable or too hard to handle, a mylar balloon ($1 at the Dollar Store) will work just as well. The gas will be saturated with water vapor.

  • 1
    $\begingroup$ This is probably a much better way to go. The humidity won't be a problem since I'll have to dilute the gas by a factor of 250 anyway to get ~4,000 ppm. I like this method very much, and feel silly not having thought of it. That's probably because I haven't actually had a carbonated beverage out of a bottle or can in years. Sad. :-) $\endgroup$
    – uhoh
    Jan 30, 2018 at 4:23

Your Answer

By clicking “Post Your Answer”, you agree to our terms of service and acknowledge that you have read and understand our privacy policy and code of conduct.

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