00:01
The types of acids that you could get.
So, these are where, what type of acid it might be.
00:08
First you have Volatile acids.
00:11
Volatile acids are primarily carbon dioxide.
00:14
So, you don’t always think of carbon dioxide
as an acid but it really is.
00:19
It fits in to the carbonic
and hydrase equation
and if you have CO2 plus
water, forms carbonic acid
and then, will this associate into hydrogen ion
and a bicarb. That process is acidic.
00:38
So, carbon dioxide in this
case is acting like an acid.
00:43
Non- volatile acids, these are stabler
but these are harder for the body to deal with.
00:49
A volatile acid is easy for the body
to deal with. You just blow off CO2.
00:55
But a Non- volatile acid has to be not only
taking care of but usually at the level of the kidney.
01:02
We have things like sulfuric acid, phosphoric acid
and you even have some organic acids
associated with different types of amino acids.
01:13
You have a very small amounts
of bases that are added to the system.
01:17
This is mainly from your gastrointestinal tract.
01:21
You do have buffers. Buffers
are going to be very important.
01:27
You can hold on to a hydrogen
ion or release it as a buffer.
01:32
So it really acts to stabilize
the pH in a narrower range.
01:38
Our big buffers that we use in
the body; the first one is bicarbonate.
01:43
And bicarbonates going to be
circulating around the blood,
it’s going to bind majority
of the hydrogen ions.
01:50
but we also do have some
non- bicarb base buffers.
01:53
Things like phosphates, things like proteins
these can also buffer hydrogen ions.
02:00
Probably, not as important as bicarb
but it’s part of the overall buffering process.
02:07
And so, we need to discuss them.
02:09
Some cells we utilize by certain buffering
techniques or types more than others.
02:18
So, let’s just go through
a couple example pH changes.
02:22
This way we can get a better insight into how the
pH will change when you add an acid or add a base.
02:31
So, let’s first add an acid.
02:33
So let’s say we add a certain
amount of an acid to a beaker.
02:37
Then we wait until that
particular beaker equilibrates.
02:43
In this case, you’ll see that
there are more hydrogen ions around
which will decrease the pH.
02:50
In our example here of the acid
that was added, we lowered pH by 0,03.
02:57
It doesn’t seem like a big pH change, right?
0,03 it’s not even 1 right?
But think arterial blood needs to have
a pH at 7,4 plus or minus (±) 0,05.
03:13
So a 0,3 change could take
it out of homeostatic normal.
03:20
If we add now a base, rather than
an acid, we put it in to our beaker,
we sit in let it equilibrate
and we have an end solution.
03:31
We take the pH of that and we
maybe give a ph change of an increase of 3.
03:38
Again, it doesn’t seem like
a much to have a 0,3 increase.
03:42
But again, that can take you
out of your homeostatic normal.
03:46
And therefore, you would
be in an alkalimic condition.
03:52
So, whether you add
an acid or add a base,
you have to think about how
that is going to change your pH.
04:01
What acids could we add?
Well, you could add a volatile one like CO2.
04:07
You can add a non- volatile one like something
like a sulfuric acid or from uric acid.
04:13
But if you want to do something like add a base,
therefore it’s probably coming from the GI tract
but it’s gonna be something with
an OH kind of group attached to it.