## The tragedies of marine towns

On monday a study by the Convention on Biological Diversity in collaboration with the UNEP World Conservation Monitoring Centre was released (->press release). The study with the title “Scientific Synthesis of the Impacts of Ocean Acidification on Marine Biodiversity” is a survey on the current results in the investigation of ocean acidity. It is thus a follow-up study to studies initiated e.g. by the global network of science academies (see IAP statement on ocean acidification ) or like the ones which led to the Monaco Declaration.

A main message of these studies and statements is that Carbondioxide i.e CO2 (a major greenhouse gas) has increasingly been taken up by the worlds oceans and thus reduced the effects caused by an increased CO2 level in the athmosphere like e.g. the greenhouse effect. This may on the first sight sound good to climate sceptics since it means that there are processes which act naturally against higher CO2 levels. Unfortunately there are now plenty of measurements which indicate that the uptake of CO2 has been slowing down in the last years, i.e. that it seems that a kind of saturation has been partially/will be reached soon. Due to this the
accumulation of CO2 in the atmosphere may accelerate rather soon.

A second main message/problem with this uptake of CO2 is If CO2 reacts with water this gives carbonic acid , which dissolves mostly to HCO3- and hydrogen ions H+. Thus after CO2 has been taken up by the ocean waters it will give to a smaller amount carbonic acid H2CO3 and carbonate ions CO3^2- and for the most part bicarbonite ions HCO3-. The hydrogen ions decrease the PH level – (you may sometimes find information of PH levels on your liquid soap) that is – the PH gives an indication of the concentration of hydrogen ions H+ via the concentration of Hydronium and it is thus a measure of the acidity or basicity of a solution.

Furthermore the carbonate ions CO3^2- form together with H+ again bicarbonate HCO3-. A higher concentration of H+ (“the acidity”) thus decreases the availablity of carbonate. But carbonate is necessary for producing calcium carbonate (CaCO3) which is essential for shell formation in marines organisms such as corals, shellfish and marine plankton. In other words the increasing acidification of the oceans is harmful to a lot of marine creatures. Since this process is very fast and the fast increasing acidification is clearly measurable this will lead to a rapid change in the composition of the oceans with more or less forseeable consequences. In particular it is very likely that this will have an impact on fish consumption.

Here is more on how the composition of oceans may change, which indicates that at least some of the marine creatures which build shells might still keep their ability to create shells despite increasing acidification. There is a new study:
Proton pumping accompanies calcification in foraminifera (via wattsupwiththat.com) which indicates that amongst others a species called perforate foraminifera Ammonia sp. seems to be able to do so and the amount of perforate foraminifera is not too small:

“A large portion of open ocean calcium carbonate production, between 20 and 50%, derives from perforate foraminifera. Despite its clear importance for the global carbon cycle, the physiological processes responsible for calcification in foraminifera are poorly understood. The key to understanding foraminiferal calcification centres on the relation between carbon speciation in seawater and preferential uptake of these chemical species (CO2, bicarbonate and/or carbonate ions)”

The mechanism is roughly the following. Foraminifera are massively pumping protons (i.e. H+) into their local environment and so make the surrounding waters even more acidic (i.e. lower PH values). This however means that on average less CO2 is dissolved in water, i.e. some of the protons will recombine with HCO3- to H2O and CO2:

Karbonatsystem_Meerwasser_de.svg by Wikipedia User:BeAr, public domain

It seems an enzym called V-type H+ ATPase is responsible for the proton pumping.
While the protons are pushed out, there is an “inside” location in the forminifer (the socalled site of calcification (SOC)) which is less acidic and so shell formation can take place. For this the CO2 is “sucked into the foraminifer”, i.e.: “As CO2 diffuses easily across cell membranes compared to HCO3−, the large pCO2 gradient results in a flux of carbon dioxide into the foraminifer.” And so shell formation can take place at the SOC via the in the blogpost described process.

How acidic is the corresponding pumped microenvironment? The researchers write:

The foreseen reduction in pH (from 8.1 today to ∼7.8 at the end of the twenty-first century36) by increased oceanic CO2 uptake is relatively small compared with the pH decrease in the foraminiferal microenvironment (down to 6.9 in Fig. 1) during calcification.

and so

Hence, a relatively moderate decrease in pH may not impair foraminiferal calcification, especially as DIC increases at the same time. Ocean acidification may still affect calcification indirectly (for example, through altered metabolism).

where DIC is “dissolved inorganic carbon” i.e. all those bi,di, etc. carbonates.

Hence in the abstract they conclude:

…total dissolved CO2 may not reduce calcification, thereby potentially maintaining the current global marine carbonate production.

which I find a bit too optimistic in view that only between 20 and 50% calcium carbonate production derives from perforate foraminifera and not much is known about the other species apart from the fact that some seem definitely not able to maintain shell formation:

Results from culturing experiments mimicking ocean acidification showed contrasting responses of calcification: calcification was reduced in some species, whereas others were not affected.

Moreover the proton pumping mechanism may not work if acidification levels lower beyond 6.9.

### 2 Responses to “The tragedies of marine towns”

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you can use LaTeX in your math comments, by using the $shortcode: [latex] E = m c^2$