<p>Yes, according to <a href="http://www.pnas.org/content/103/38/14164.full" rel="nofollow noreferrer">this paper in the Proceedings of the National Academy of Sciences</a>. But they also say that this "lake" of liquid CO<sub>2</sub> is covered by <a href="http://en.wikipedia.org/wiki/Carbon_dioxide_clathrate" rel="nofollow noreferrer">CO<sub>2</sub> clathrate</a>, so it's not quite your <a href="http://en.wikipedia.org/wiki/Brine_pool" rel="nofollow noreferrer">average brine pool</a>.</p>

<p><strong>Note about clathrates:</strong></p>

<p>The following image is from the <a href="http://en.wikipedia.org/wiki/Carbon_dioxide_clathrate" rel="nofollow noreferrer">Wikipedia article on CO<sub>2</sub> clathrate</a>. It is a CO<sub>2</sub> hydrate P-T phase diagram with experimental data (black squares) from a 1998 paper by Sloan listed in the <a href="http://en.wikipedia.org/wiki/Carbon_dioxide_clathrate#References" rel="nofollow noreferrer">references</a> of the Wikipedia article.<img src="https://i.sstatic.net/LmJQK.jpg" alt="Sloan 1998 CO&lt;sub&gt;2&lt;/sub&gt; hydrate phase diagram"></p>

<p>Note the H<sub>2</sub>O phase lines drawn in. There is a relatively small habitable area for clathrate somewhere inside about 273-280 K (0-7 ºC) and 10-12 bar (or about 90-110m in ocean depth as calculated <a href="http://www.calctool.org/CALC/other/games/depth_press" rel="nofollow noreferrer">here</a>). Above the phase boundary, the clathrate will dissolve to liquid. Below, to gas. What this diagram does not say (according to a knowledgeable colleague) is that clathrate will not readily form or remain in its semi-organized state given very slight amounts of mechanical agitation. Hence why it does not exist en masse under typical seafloor conditions. </p>

CC BY-SA 3.0
2015-05-20T05:10:21.220Z
Why these lakes are so rare? Given the amount of CO2 in atmosphere, all ocen floors should be covered with liquid CO2.
Anixx
CC BY-SA 3.0
2015-05-20T18:00:12.733Z
@Anixx: Why?  Assuming liquid CO2 is somewhat soluble in water, then any lakes would slowly dissolve into the ocean when they come into contact with water.  Similarly, you might ask why there are no solid salt deposits in the ocean.
jamesqf
CC BY-SA 3.0
2015-05-20T20:59:17.260Z
According to a colleague of mine, semi-organized clathrate-state CO2 pockets are extremely vulnerable to transformation back to their gaseous state if they are physically disturbed, in which case they would quickly escape to the surface as gas bubbles. This could be why you don't see more of them around.
Ian
CC BY-SA 3.0
2015-05-20T21:07:06.823Z
Or, more likely, travel upwards as gas until partially or completely dissolved into solution.
Ian
CC BY-SA 3.0
2015-05-21T05:14:48.347Z
Why would they become gas if on the phase diagram CO2 should be liquid at this pressure?
Anixx
CC BY-SA 3.0
2015-05-21T09:54:29.437Z
@Anixx please check the updated answer. I should have commented that they are vulnerable to transformation back to their gaseous or liquid states.
Ian
CC BY-SA 3.0
2016-05-05T11:27:27.917Z
@Anixx Those are idealized models. In reality, a bit of stuff doesn't have a tag that it's either "liquid" or "gas" (or another phase) - it's just a useful way to model stuff, not a physical reality. Introduce disruptions into such a lake, and you'll get a mix of water vapour, carbon dioxide, carbonix acid, some of them "liquid", some "gaseous", and who knows what else. Fringes are especially tricky, and your scenario is very much on the fringe here.
Luaan
CC BY-SA 3.0
2015-05-20T02:05:09.733Z
2016-05-02T15:14:16.810Z
2016-05-02T15:14:16.810Z
Ian
<p>There are several reasons why the ocean floor is not a pool of liquid $\ce{CO_2}$:</p>

<ol>
<li><p>Solubility of gaseous $\ce{CO_2}$ in brine is low.  </p></li>
<li><p>Mass transfer of gaseous $\ce{CO_2}$ from the atmosphere is slower than the time to react with water to make carbonate/bicarbonate</p></li>
<li><p>Carbonate/bicarbonate act as a buffer for atmospheric $\ce{CO_2}$ precipitating and dissolving as atmospheric $\ce{CO_2}$ fluctuates.  </p></li>
</ol>

<p>Liquid $\ce{CO_2}$ at the ocean floor must have a source of pure enough $\ce{CO_2}$ to liquefy and it must be in enough abundance, at a high enough pressure, so that it is not diluted or mixed with water or brine.</p>

<p>The data above shows that this has happened somewhere in the world... that is cool.</p>

CC BY-SA 3.0
2015-07-28T17:51:46.337Z
2015-07-28T19:54:15.030Z
2015-07-28T19:54:15.030Z
JonT
<p>The carbon dioxide phase diagram shows that at high pressure and normal temperature CO<sub>2</sub> becomes liquid. Since it is heavier than water, I wonder if there are lakes of liquid CO<sub>2</sub> at the bottom of the Earth's oceans, and if no, why?</p>

<p><img src="https://i.sstatic.net/oB0oS.gif" alt="enter image description here"></p>

CC BY-SA 3.0
2015-05-19T22:46:24.983Z
Quick answer is no, however there are methane clathrates somewhere down there and possibly also carbon dioxide clathrates as well. Waiting for someone with better knowledge of the subject to answer it...
Gimelist
CC BY-SA 3.0
2015-05-21T01:47:26.787Z
it looks like, and it's hard to tell precisely just looking at the chart, but at 4 degrees C - about the temperature of the deep ocean, it looks like that would require over 1,000 ATMs (33,000 feet).   It looks to me, looking at the chart, that even the deepest part of the ocean wouldn't have sufficient temperature/pressure combo to liquify CO2.   If the oceans were twice or three times as deep - then it might be possible.   Europa just might have pools of liquid CO2 . . . maybe.  Maybe not with it's lower gravity.  Mixing would also be a factor.
userLTK
CC BY-SA 3.0
2015-05-21T03:25:07.340Z
Isn't that diagram very misleading? It's for pure CO2. There must be a diagram for CO2-H2O-NaCl somewhere.
Mark Rovetta
CC BY-SA 3.0
2015-05-21T05:29:14.787Z
It's a standard phase diagram, so I don't think it's meant to be misleading.    I think Anixx' question is, in essence, since CO2 can be a liquid under temperature and pressure similar to what exists deep in the ocean is liquid CO2 possible in the ocean.   My hunch is no as it would just mix and stay dissolved in the H20, not separate.   CO2 in H20 also sometimes becomes H2CO3 which is also prone to lend an H+ to an H20 and create light acidity - one of the problems we're having with greenhouse gas.    I've also never seen a phase diagram for a mix of elements.   It would be more complicated
userLTK
CC BY-SA 3.0
2015-05-21T05:34:26.080Z
@userLTK dissolution is possible only up to certain concentration, and there is a lot of CO2 available.
Anixx
CC BY-SA 3.0
2015-05-21T06:00:39.550Z
I'm not a chemistry guy but there's a lot lot lot more water than there is CO2.   If the atmosphere was cooled to a liquid and the same density as water, it would be 33 maybe 34 feet high and at 400 parts per million, (1 part in 2,500), all the CO2 in the atmosphere, if liquified would be 1/2 centimeter high.    That's not very much compared to the oceans which average 1.5 miles in depth.   There's also this:   http://www.jochemnet.de/fiu/CO2Cycle.jpg  it tends to not stay CO2, it interacts with the water and Calcium in the lower ocean.
userLTK
CC BY-SA 3.0
2015-05-21T06:14:26.383Z
@userLTK still there is a lot of CO2 in atmosphere and it is said to exceed the amount the oceans can dissolve.
Anixx
CC BY-SA 3.0
2015-05-21T07:06:13.167Z
@Anixx the concentration of CO2 in the atmosphere and in the ocean in somewhere between 300 and 800 ppm -> that's part per million. It is a lot but it still is comparatively a low concentration.
plannapus
<ocean><oceanography><carbon>
Are there pockets of liquid carbon dioxide in Earth's oceans?
Anixx
# Are there pockets of liquid carbon dioxide in Earth's oceans?

(Asked by: username_0 on 2015-05-19)

The carbon dioxide phase diagram shows that at high pressure and normal temperature CO2 becomes liquid. Since it is heavier than water, I wonder if there are lakes of liquid CO2 at the bottom of the Earth's oceans, and if no, why?

![enter image description here](https://i.sstatic.net/oB0oS.gif)

**Tags:** ocean, oceanography, carbon

> **Comments:**
> **username_1**: Quick answer is no, however there are methane clathrates somewhere down there and possibly also carbon dioxide clathrates as well. Waiting for someone with better knowledge of the subject to answer it...  
> **username_2**: it looks like, and it's hard to tell precisely just looking at the chart, but at 4 degrees C - about the temperature of the deep ocean, it looks like that would require over 1,000 ATMs (33,000 feet).   It looks to me, looking at the chart, that even the deepest part of the ocean wouldn't have sufficient temperature/pressure combo to liquify CO2.   If the oceans were twice or three times as deep - then it might be possible.   Europa just might have pools of liquid CO2 . . . maybe.  Maybe not with it's lower gravity.  Mixing would also be a factor.  
> **username_3**: Isn't that diagram very misleading? It's for pure CO2. There must be a diagram for CO2-H2O-NaCl somewhere.  
> **username_2**: It's a standard phase diagram, so I don't think it's meant to be misleading.    I think username_0' question is, in essence, since CO2 can be a liquid under temperature and pressure similar to what exists deep in the ocean is liquid CO2 possible in the ocean.   My hunch is no as it would just mix and stay dissolved in the H20, not separate.   CO2 in H20 also sometimes becomes H2CO3 which is also prone to lend an H+ to an H20 and create light acidity - one of the problems we're having with greenhouse gas.    I've also never seen a phase diagram for a mix of elements.   It would be more complicated  
> **username_0**: @username_2 dissolution is possible only up to certain concentration, and there is a lot of CO2 available.  
> **username_2**: I'm not a chemistry guy but there's a lot lot lot more water than there is CO2.   If the atmosphere was cooled to a liquid and the same density as water, it would be 33 maybe 34 feet high and at 400 parts per million, (1 part in 2,500), all the CO2 in the atmosphere, if liquified would be 1/2 centimeter high.    That's not very much compared to the oceans which average 1.5 miles in depth.   There's also this:   http://www.jochemnet.de/fiu/CO2Cycle.jpg  it tends to not stay CO2, it interacts with the water and Calcium in the lower ocean.  
> **username_0**: @username_2 still there is a lot of CO2 in atmosphere and it is said to exceed the amount the oceans can dissolve.  
> **username_4**: @username_0 the concentration of CO2 in the atmosphere and in the ocean in somewhere between 300 and 800 ppm -> that's part per million. It is a lot but it still is comparatively a low concentration.  

---

## 2 answers

### Answer by username_5 on 2015-05-20. Score: 13

Yes, according to [this paper in the Proceedings of the National Academy of Sciences](http://www.pnas.org/content/103/38/14164.full). But they also say that this "lake" of liquid CO2 is covered by [CO2 clathrate](http://en.wikipedia.org/wiki/Carbon_dioxide_clathrate), so it's not quite your [average brine pool](http://en.wikipedia.org/wiki/Brine_pool).

**Note about clathrates:**

The following image is from the [Wikipedia article on CO2 clathrate](http://en.wikipedia.org/wiki/Carbon_dioxide_clathrate). It is a CO2 hydrate P-T phase diagram with experimental data (black squares) from a 1998 paper by Sloan listed in the [references](http://en.wikipedia.org/wiki/Carbon_dioxide_clathrate#References) of the Wikipedia article.![Sloan 1998 CO<sub>2</sub> hydrate phase diagram](https://i.sstatic.net/LmJQK.jpg)

Note the H2O phase lines drawn in. There is a relatively small habitable area for clathrate somewhere inside about 273-280 K (0-7 ºC) and 10-12 bar (or about 90-110m in ocean depth as calculated [here](http://www.calctool.org/CALC/other/games/depth_press)). Above the phase boundary, the clathrate will dissolve to liquid. Below, to gas. What this diagram does not say (according to a knowledgeable colleague) is that clathrate will not readily form or remain in its semi-organized state given very slight amounts of mechanical agitation. Hence why it does not exist en masse under typical seafloor conditions.

> **Comments:**
> **username_0**: Why these lakes are so rare? Given the amount of CO2 in atmosphere, all ocen floors should be covered with liquid CO2.  
> **username_6**: @username_0: Why?  Assuming liquid CO2 is somewhat soluble in water, then any lakes would slowly dissolve into the ocean when they come into contact with water.  Similarly, you might ask why there are no solid salt deposits in the ocean.  
> **username_5**: According to a colleague of mine, semi-organized clathrate-state CO2 pockets are extremely vulnerable to transformation back to their gaseous state if they are physically disturbed, in which case they would quickly escape to the surface as gas bubbles. This could be why you don't see more of them around.  
> **username_5**: Or, more likely, travel upwards as gas until partially or completely dissolved into solution.  
> **username_0**: Why would they become gas if on the phase diagram CO2 should be liquid at this pressure?  
> **username_5**: @username_0 please check the updated answer. I should have commented that they are vulnerable to transformation back to their gaseous or liquid states.  
> **username_7**: @username_0 Those are idealized models. In reality, a bit of stuff doesn't have a tag that it's either "liquid" or "gas" (or another phase) - it's just a useful way to model stuff, not a physical reality. Introduce disruptions into such a lake, and you'll get a mix of water vapour, carbon dioxide, carbonix acid, some of them "liquid", some "gaseous", and who knows what else. Fringes are especially tricky, and your scenario is very much on the fringe here.  

---

### Answer by username_8 on 2015-07-28. Score: 5

There are several reasons why the ocean floor is not a pool of liquid $\ce{CO\_2}$:

1. Solubility of gaseous $\ce{CO\_2}$ in brine is low.
2. Mass transfer of gaseous $\ce{CO\_2}$ from the atmosphere is slower than the time to react with water to make carbonate/bicarbonate
3. Carbonate/bicarbonate act as a buffer for atmospheric $\ce{CO\_2}$ precipitating and dissolving as atmospheric $\ce{CO\_2}$ fluctuates.

Liquid $\ce{CO\_2}$ at the ocean floor must have a source of pure enough $\ce{CO\_2}$ to liquefy and it must be in enough abundance, at a high enough pressure, so that it is not diluted or mixed with water or brine.

The data above shows that this has happened somewhere in the world... that is cool.


---

