<p>If it rains hard enough it will completely strip the atmosphere of CO<sub>2</sub> in that area.
A very simple experiment can chart the CO<sub>2</sub> captured by rain droplets in relation to
the intensity of the rain over time.  Once it's done raining the replenishment of CO<sub>2</sub>
in the depleted area is fairly quick.  It takes about 3 minutes 30 seconds for the CO<sub>2</sub>
to evolve. The evolution from start to finish it's a deceleration event.
Hope this helps everyone out.</p>

CC BY-SA 4.0
2019-10-11T21:57:11.947Z
Can you add references? That would be great, since it contradicts other answers.
Jan Doggen
CC BY-SA 4.0
2019-10-16T15:33:10.177Z
About 3 yrs. ago MIT was conducting their own experiments on this exact topic.  It was to better pinpoint the absorption rate of aerosols in a droplet of water falling through the atmosphere.  The Earth is like a huge wet scrubber.  If a person understands how a scrubber works it's easier to imagine what is happening with rain and atmosphere.  Collect the first 100 ml of rain in a rain storm and immediately put the ph meter in the water.  You should see a TDS of 10 to 20 and a ph of less than 7
Brian
CC BY-SA 4.0
2019-10-16T15:51:39.407Z
What exactly that ph reading might be depends on the elevation that the droplet started at.  In the first 30 seconds of that sample the ph will come down fairly fast.  Collect a 100 ml of the last of the rain in the same rain storm.  If it reads 7 on the ph meter than the co2 is gone.  When it comes to knowing the exact numbers, no one knows.  Elevation, droplet size, droplet quantity and duration all play a roll.  Each rain storm can yield a slightly different result because of these factors.
Brian
CC BY-SA 4.0
2019-10-11T21:21:01.600Z
2021-02-13T06:26:15.607Z
2021-02-13T06:26:15.607Z
Brian
<p>I appreciate all of the thoughtful responses above and for the mathematical understanding that I personally would not have about this topic. One factor that may not have been considered in this discussion is the association of CO2 and water in the atmosphere and how this may have a significant affect on increasing the CO2 integration in raindrops. Another factor that must be considered is in the presence of competing organic and inorganic matter suspended in the atmosphere. Raindrops form not as a simple threshold reached between temperature,  barometric pressure and water content. We need to first differentiates free water versus bound water . In addition, we have to consider the concentration of ice nucleating Protein present on the membranes of bacteria suspended in the atmosphere. These catalysts are key in initiating the water droplet formation. Bacteria that utilize this process to return to earth are carbon fixers and also help slow evaporation. Water cycle is a part of life or better yet, it is life. Not knowing all of these specific factors and not having the mathematical knowledge I don’t think I would ever be able to figure this problem out. However, I used to live in Los Angeles. The visual  effect of a rainfall transforming smog to clear blue skies and seeing the snow capped mountains once or twice a year tells me there must be something more here.</p>

CC BY-SA 4.0
2022-05-27T04:26:55.307Z
2022-05-27T04:26:55.307Z
Kourosh Bagheri
<p>Here is the mass-calculation. We will consider a column of the atmosphere with a footprint of 1m × 1m. This column weighs about 10,000 kg (per square metre). In these days of climate change we will assume the current average CO<sub>2</sub> concentration is 400 ppm, yielding a total mass of CO<sub>2</sub> in this column of 4 kg. 
The rain doesn't wash out the entire thickness of atmosphere but only (in general) the lowermost troposphere. We will assume, generously, that some 2.5 kg of this 4 kg of CO<sub>2</sub> is available to be scavenged by raindrops. 
Now consider a cloudburst of raindrops, equivalent to some 100 mm  on the ground. So we have 0.1 cubic metres, or 100 kg, of fallen raindrops within our square metre column of air. The solubility of CO<sub>2</sub> in air is strongly temperature dependent, up to 2.5 g per kg at 10 deg C. But at such a low temperature we couldn't achieve 100 mm of rainfall, so we will compromise at about 1.5 g per kg at 25 °C. So, assuming complete CO<sub>2</sub> saturation within the raindrops (unlikely) our 100 kg of rain will contain 0.15 kg of CO<sub>2</sub> , scavenged from about 2.5 kg of CO<sub>2</sub> in the 'rained out' column of air, or about 6% of the low atmospheric CO<sub>2</sub> . </p>

<p>Bear in mind that this assumes an enormous rainfall intensity, 100% CO<sub>2</sub> saturation of the water and equilibrium chemical dynamics. After the raindrops hit the ground at least half of it will immediately re-evaporate back into the air, leaving, at absolute most, about 3% of the atmospheric CO2 leached out of the atmosphere that will be available to react with the soil, rock or biosphere. Also consider that this is but one of several important processes affecting CO<sub>2</sub> transience, such as photosynthesis, respiration, volcanism, industrial pollution, etc. So the CO<sub>2</sub> estimates that you read about are average values. Advection and turbulent air mixing should ensure that the CO<sub>2</sub> regains approximately normal concentration within an hour or two after rainfall. </p>

CC BY-SA 3.0
2015-11-17T20:00:10.513Z
The 'hour or two' is not pure speculation, it is a rough estimate based upon a typical duration of rain-storm and footprint size, and a typical advection rate of replacement air. There are so many variables that it is pointless to try to be more precise. The back of an envelope calculation is not meant to be precise, but is sufficient to demonstrate that rain cannot greatly affect the CO2, even under extreme conditions.
Gordon Stanger
CC BY-SA 3.0
2015-11-18T00:08:48.943Z
There are estimates posted above that CO2 by PPM in a rain-drop is about 355, so 1 KG of rain using 355 PPM estimate, is about .355 grams (equivalent) and when we adjust for molecular weight, about .87 grams CO2 per KG of rain.   Your estimate, 1.5 g per KG isn't too far off, but it's nearly twice the actual amount.    Something else to consider, especially in warmer temperatures, a share of rain water evaporates so a share of that CO2 is fairly quickly returned to the atmosphere.   Props for working out the calculation though.
userLTK
CC BY-SA 3.0
2015-11-18T07:32:41.593Z
ppm is not mass%
mart
CC BY-SA 3.0
2015-11-19T03:06:01.363Z
@mart I did that.   That's why it went from .355 grams (equivalent) to .87 grams (real).   CO2 being about 2.4 times the mass of H20.
userLTK
CC BY-SA 3.0
2015-11-19T04:00:10.413Z
355, 400 ppm? Who gives a stuff? - it's just a back of an envelope calculation to demonstrate that the scale of CO2 scavenging by rain is trivially small.
Gordon Stanger
CC BY-SA 3.0
2015-11-17T15:22:39.633Z
2016-09-14T10:48:26.757Z
2016-09-14T10:48:26.757Z
Gordon Stanger
<p>CO<sub>2</sub> in the air dissolves into rain water, making them slightly acidic. Is that enough to deplete the surrounding air out of CO<sub>2</sub>? If yes, how fast does this occur? Is it only with the first drops of rain or do you need several hours?</p>

<p>How long does it take for the surrounding atmosphere to regain its original CO<sub>2</sub> contents, assuming this actually happens?</p>

CC BY-SA 3.0
2015-11-17T09:59:27.793Z
I would have thought that the CO2 would be dissolved as the cloud formed, rather than as it rained, and hence there would be plenty of time for the mixing of the atmosphere to even out any changes in concentration, but that is just my intuition.  Interesting question.
Dikran Marsupial
CC BY-SA 3.0
2015-11-17T10:51:43.837Z
the dimensionless Henrey constant is something about 0,83 so you have 0,83 x 400 ppm = 332 ppm CO2 in the water. give nthat the molar concentration in water and air is almost the same but the air column is very very high compared to the liquid water volume I'd say the effect on the athmosphere is small to rediculosly small.
mart
CC BY-SA 3.0
2015-11-17T23:55:29.953Z
@mart  nice estimate.   I found two websites that suggest the number 355 PPM.   Here http://www.ehow.com/info_12300030_much-co2-rain-water.html and here: http://www.chemistry.wustl.edu/~edudev/LabTutorials/Water/FreshWater/acidrain.html  Given that water vapor is rarely more than 3% of the atmosphere and only a fraction of that can turn into rain, and the PPM is slightly lower in rain-water than air, that's a pretty slow way of pulling CO2 from the atmosphere.   what's more, as rain water evaporates, that CO2 is returned to the atmosphere.
userLTK
<meteorology><atmosphere><carbon><co2><rain>
Does rain (temporarily) deplete the surrounding atmosphere of carbon dioxide?
Gimelist
# Does rain (temporarily) deplete the surrounding atmosphere of carbon dioxide?

(Asked by: username_0 on 2015-11-17)

CO2 in the air dissolves into rain water, making them slightly acidic. Is that enough to deplete the surrounding air out of CO2? If yes, how fast does this occur? Is it only with the first drops of rain or do you need several hours?

How long does it take for the surrounding atmosphere to regain its original CO2 contents, assuming this actually happens?

**Tags:** meteorology, atmosphere, carbon, co2, rain

> **Comments:**
> **username_1**: I would have thought that the CO2 would be dissolved as the cloud formed, rather than as it rained, and hence there would be plenty of time for the mixing of the atmosphere to even out any changes in concentration, but that is just my intuition.  Interesting question.  
> **username_2**: the dimensionless Henrey constant is something about 0,83 so you have 0,83 x 400 ppm = 332 ppm CO2 in the water. give nthat the molar concentration in water and air is almost the same but the air column is very very high compared to the liquid water volume I'd say the effect on the athmosphere is small to rediculosly small.  
> **username_3**: @username_2  nice estimate.   I found two websites that suggest the number 355 PPM.   Here http://www.ehow.com/info_12300030_much-co2-rain-water.html and here: http://www.chemistry.wustl.edu/~edudev/LabTutorials/Water/FreshWater/acidrain.html  Given that water vapor is rarely more than 3% of the atmosphere and only a fraction of that can turn into rain, and the PPM is slightly lower in rain-water than air, that's a pretty slow way of pulling CO2 from the atmosphere.   what's more, as rain water evaporates, that CO2 is returned to the atmosphere.  

---

## 3 answers

### Answer by username_7 on 2015-11-17. Score: 16 | Accepted answer

Here is the mass-calculation. We will consider a column of the atmosphere with a footprint of 1m × 1m. This column weighs about 10,000 kg (per square metre). In these days of climate change we will assume the current average CO2 concentration is 400 ppm, yielding a total mass of CO2 in this column of 4 kg.
The rain doesn't wash out the entire thickness of atmosphere but only (in general) the lowermost troposphere. We will assume, generously, that some 2.5 kg of this 4 kg of CO2 is available to be scavenged by raindrops.
Now consider a cloudburst of raindrops, equivalent to some 100 mm on the ground. So we have 0.1 cubic metres, or 100 kg, of fallen raindrops within our square metre column of air. The solubility of CO2 in air is strongly temperature dependent, up to 2.5 g per kg at 10 deg C. But at such a low temperature we couldn't achieve 100 mm of rainfall, so we will compromise at about 1.5 g per kg at 25 °C. So, assuming complete CO2 saturation within the raindrops (unlikely) our 100 kg of rain will contain 0.15 kg of CO2 , scavenged from about 2.5 kg of CO2 in the 'rained out' column of air, or about 6% of the low atmospheric CO2 .

Bear in mind that this assumes an enormous rainfall intensity, 100% CO2 saturation of the water and equilibrium chemical dynamics. After the raindrops hit the ground at least half of it will immediately re-evaporate back into the air, leaving, at absolute most, about 3% of the atmospheric CO2 leached out of the atmosphere that will be available to react with the soil, rock or biosphere. Also consider that this is but one of several important processes affecting CO2 transience, such as photosynthesis, respiration, volcanism, industrial pollution, etc. So the CO2 estimates that you read about are average values. Advection and turbulent air mixing should ensure that the CO2 regains approximately normal concentration within an hour or two after rainfall.

> **Comments:**
> **username_7**: The 'hour or two' is not pure speculation, it is a rough estimate based upon a typical duration of rain-storm and footprint size, and a typical advection rate of replacement air. There are so many variables that it is pointless to try to be more precise. The back of an envelope calculation is not meant to be precise, but is sufficient to demonstrate that rain cannot greatly affect the CO2, even under extreme conditions.  
> **username_3**: There are estimates posted above that CO2 by PPM in a rain-drop is about 355, so 1 KG of rain using 355 PPM estimate, is about .355 grams (equivalent) and when we adjust for molecular weight, about .87 grams CO2 per KG of rain.   Your estimate, 1.5 g per KG isn't too far off, but it's nearly twice the actual amount.    Something else to consider, especially in warmer temperatures, a share of rain water evaporates so a share of that CO2 is fairly quickly returned to the atmosphere.   Props for working out the calculation though.  
> **username_2**: ppm is not mass%  
> **username_3**: @username_2 I did that.   That's why it went from .355 grams (equivalent) to .87 grams (real).   CO2 being about 2.4 times the mass of H20.  
> **username_7**: 355, 400 ppm? Who gives a stuff? - it's just a back of an envelope calculation to demonstrate that the scale of CO2 scavenging by rain is trivially small.  

---

### Answer by username_4 on 2019-10-11. Score: 1

If it rains hard enough it will completely strip the atmosphere of CO2 in that area.
A very simple experiment can chart the CO2 captured by rain droplets in relation to
the intensity of the rain over time. Once it's done raining the replenishment of CO2
in the depleted area is fairly quick. It takes about 3 minutes 30 seconds for the CO2
to evolve. The evolution from start to finish it's a deceleration event.
Hope this helps everyone out.

> **Comments:**
> **username_5**: Can you add references? That would be great, since it contradicts other answers.  
> **username_4**: About 3 yrs. ago MIT was conducting their own experiments on this exact topic.  It was to better pinpoint the absorption rate of aerosols in a droplet of water falling through the atmosphere.  The Earth is like a huge wet scrubber.  If a person understands how a scrubber works it's easier to imagine what is happening with rain and atmosphere.  Collect the first 100 ml of rain in a rain storm and immediately put the ph meter in the water.  You should see a TDS of 10 to 20 and a ph of less than 7  
> **username_4**: What exactly that ph reading might be depends on the elevation that the droplet started at.  In the first 30 seconds of that sample the ph will come down fairly fast.  Collect a 100 ml of the last of the rain in the same rain storm.  If it reads 7 on the ph meter than the co2 is gone.  When it comes to knowing the exact numbers, no one knows.  Elevation, droplet size, droplet quantity and duration all play a roll.  Each rain storm can yield a slightly different result because of these factors.  

---

### Answer by username_6 on 2022-05-27. Score: -1

I appreciate all of the thoughtful responses above and for the mathematical understanding that I personally would not have about this topic. One factor that may not have been considered in this discussion is the association of CO2 and water in the atmosphere and how this may have a significant affect on increasing the CO2 integration in raindrops. Another factor that must be considered is in the presence of competing organic and inorganic matter suspended in the atmosphere. Raindrops form not as a simple threshold reached between temperature, barometric pressure and water content. We need to first differentiates free water versus bound water . In addition, we have to consider the concentration of ice nucleating Protein present on the membranes of bacteria suspended in the atmosphere. These catalysts are key in initiating the water droplet formation. Bacteria that utilize this process to return to earth are carbon fixers and also help slow evaporation. Water cycle is a part of life or better yet, it is life. Not knowing all of these specific factors and not having the mathematical knowledge I don’t think I would ever be able to figure this problem out. However, I used to live in Los Angeles. The visual effect of a rainfall transforming smog to clear blue skies and seeing the snow capped mountains once or twice a year tells me there must be something more here.


---

