(gentle music) - [Narrator] Instead of global warming, these days we talk about global change. And ocean acidification
kind of worked its way into the fabric of this
change, making it possible for us to look at the
problem of global change in a more expansive way than
the more simplistic idea of global warming. But what is ocean acidification? And how exactly does it affect our topic of interest, biodiversity? First, we need to look at the
cause of ocean acidification in order to understand what it actually is and what it means to biodiversity. Essentially, if you talk
about this big cloud, this puff of CO2, that's
produced by human activity, 30 to 40%, almost half, of
that cloud ends up dissolved in the ocean. The rest stays in the
atmosphere or it's incorporated into living things in
some form or another, usually as plant material or
the bodies of other producers. But the huge amount of
CO2 that gets dissolved in the oceans is definitely
going to be doing something. The added CO2 in the ocean
causes an increase in acidity. Acidity is measured by
something called pH. And it's worth talking a little
bit about pH for a moment. A couple of things to
note about the pH scale. It goes from zero to 14
where zero is highly acidic and 14 is highly alkaline,
also called highly basic. A pH of seven is neutral
like distilled water. So if you increase
acidity, the pH is dropping and if you increase
alkalinity, the pH is going up. Note that the pH scale is logarithmic, which means that each
step is a factor of 10. If you go from a pH of six to something slightly less
alkaline, that is more acidic, at a pH of five, you're actually increasing the acidity 10 times. Going from pH six to pH
four, it's more acidic by a factor of 10 times 10, which means 100 times more acidic. Most importantly, pH is
a measure of potential. That's where the p in pH comes from. The power or potential of a liquid to make charged hydrogen atoms or ions. Think of pH as potential H
or power of hydrogen ions. We'll see in a moment why the
power of such a tiny thing as a hydrogen ion is so crucial. First, let's look at this problem of introducing carbon dioxide to seawater. Over the industrial
period between about 1751 and the early 1990s, the
surface ocean pH decreased from about 8.25 to 8.14. That doesn't sound like
a lot, but remember, we're talking about an average
for the entire global ocean over the globe and it's logarithmic. So we're actually talking
about a 30% increase in hydrogen ion
concentration in the ocean. We've got CO2 in the atmosphere
that's going into the water. The CO2 breaks down. We have a chemical reaction
where the CO2 plus the water leads to carbonic acid. The process looks like this. When you have the carbonic
acid in the water, a couple of things happen. Each carbonic acid molecule can release one of its hydrogen ions to make something called a bicarbonate. And a bicarbonate molecule
can further break down into a carbonate ion. The big issue here is you
get both of these molecules, bicarbonate and carbonate
by losing hydrogen ions, which are now zipping
around freely in the water. And remember what we
said about hydrogen ions. They're going to increase
the acidity of the water. And that's the key point. Through the addition of CO2,
you set up a chain of events that results in these
powerful little hydrogen ions being set free as the active
ingredient, or the culprit, in the damage that acids can do. It's worth talking about
this global process in terms of rate. It's not so much that the
pH levels are changing, but they're changing faster
than anything we've seen for a very long time. The current rates of
acidification are very similar to those during an
enormous greenhouse event that occurred at the
Paleocene/Eocene boundary 55 million years ago. And that time was marked
by huge extinctions at very fundamental levels
of ecosystem production, particularly in the deep sea. Geologic history tells
us that biodiversity can be threatened by
exposure to increased acidity in the oceans. There's a huge range of
harmful consequences, including drops in metabolic rate or drops in immune
response to other organisms such as parasites or bacteria
that are in the environment. And we know that drops in
pH can cause destruction of coral by triggering chemical reactions that result in an overall drop of the amount of carbonate ions available. Okay, so what does that mean? Well, it means a bit more chemistry. Many organisms that live in the ocean use a very special building
material, calcium carbonate, which is dissolved in seawater. And it's made by this reaction. Add calcium atoms to carbonate ions and you make calcium carbonate, a material that goes into
the skeletons of organisms that live in the sea, such as corals and molluscs and crabs. They're very dependent
on calcium carbonate. Unfortunately, these free carbonate ions are also recombining with those busy, very reactive hydrogen ions
to make more bicarbonate. So this reduces the
available calcium carbonate that organisms would
otherwise be able to use. And that means that organisms with a calcium carbonate skeleton are going to have trouble
maintaining their skeleton simply because they can't get enough of the calcium carbonate to grow or repair their shells and skeletons. It turns out that it's
not just corals, molluscs, and crabs that are affected. Single-celled organisms called foraminifera and coccolithophores which are close to the
base of the food web and terribly important
in marine ecosystems are among the most effected. If you put a foraminiferan, or foram, under a microscope, they
look like little spirals and funny-shaped boxes. They're fantastic things to look at. Forams are like little
single-celled amoebae that make shells. They're metabolism and
ability to make those shells is deeply affected by
pH levels in the ocean. Now, coccolithophores
are really interesting, somewhat mysterious, single-celled algae that also take up calcium
carbonate from the ocean to make a coccolith. Lith means rock and cocco
roughly means berry-shaped. So these organisms are
shaped like tiny fruit, but with a rocky covering. Not everyone knows about
these, but now you do. Because they're plants,
they are really important as phytoplankton producers
in ocean ecosystems. No one's too sure why they make their calcium carbonate coverings, but the mere fact that they are making their calcium carbonate shells means that they're also going
to be deeply affected by decreasing oceanic pH. And there've always been lots
and lots of coccolithophores. The White Cliffs of Dover
are made up almost entirely of fossil coccoliths. Coccolithophores produce a
chemical that contributes to the formation of clouds. Some scientists even think
that threatening the existence of coccolithophores could
result in a reduction in cloud cover over the oceans,
reducing the reflectivity of the earth and, thereby,
increasing the rate of global warming. As I mentioned, bigger
things like corals and crabs and snails and clams will
also have some issues with their ability to
secrete calcium carbonate. They depend so much on that. Scientists have run experiments in which increasing the amount of
CO2 in the air above a tank of seawater can actually increase the rate at which the skeletons of some of these forams will dissolve. Now, notice I said some. It's variable, but we're
seeing some effects in almost every major group of organisms that we've looked at so
far, even in starfish and sea urchins which have protective skin over their entire bodies. They actually have an
internal skeleton like fish or you or me, but even
those have problems, particularly in larval stages. And these larvae form a
huge part of the plankton and remember how crucial
plankton are to food webs in the sea. Even for organisms that
don't have calcium carbonate skeletons and shells, increased
acidity can be a problem. Hypercapnia, which is
an actual excess of CO2 in the body fluids of
organisms, can happen in things like fish or squid and mess
with their immune responses. Excess CO2 can even make it
difficult for baby clown fish to distinguish among the
odors of friends and foes and interfere with sensory mechanisms or even the ability to
hear predators coming. The latter is kind of interesting because you can get changes
in the acoustic properties of seawater by changing its chemistry and that has huge
implications for any animal that uses echolocation, for example. CO2 increases ocean noise,
which is already getting noisier all the time through
other human activities. More acidic environments can interfere with the construction
of things like ear bones and balance organs, such as
what are known as statoliths, tiny little stones that
squid make and hold in special chambers in their bodies. Statoliths allow squid to
sense pressure and changes in direction and movement. And this just illustrates
how little we know. Things have unusual kinds
of cascading effects that you might not think of
over and above this inability to make calcium carbonate
skeletons from seawater. Here's another example that
has a complicated story. Like land plants,
seagrasses do a bit better in building their bodies when
CO2 levels are increased. And seagrasses are really important. They're valuable feeding
and spawning sites for a variety of species so
if you enhance the growth of seagrasses, maybe you're
doing something good? But what we don't know is
if those local benefits of better seagrass
growth will be outweighed by the wider disruption to the
marine food chain as a whole and what that means for biodiversity. These are all pretty complicated things. We don't really know what the longterm or even short-term interplay
of all these different factors is going to be. We definitely need some focused
research on these topics. But we do know that ocean
acidification is certainly mostly bad news. It's a global problem
and we're going to need to start talking about global
solutions as soon as possible. (gentle music)