vivianimbriotis | Feb. 2, 2025, 1:46 a.m.
Do not read this to try to learn acid-base physiology. This is not good didactic content. This is the product of a disturbed and pathological mind. This will be your only warning.
Every moment, you body is trying to kill you. Every molecule of ATP your cells hydrolyze, every amino acid you metabolize, generates acid. There are three systems that prevent you from drying from acidosis:
The acid-base status is determined by the chemical activity of hydrogen in the extracellular fluid. This is determined by a number of interrelated quantities.
To understand this we first need to understand some prerequisites:
Then we will need to understand the regulators of these parameters, which are
There are three approaches to measuring these variables to try and determine the cause of an acid base disturbance
The rate of change of CO2 is the rate of generation of CO2, minus the rate of excretion of CO2.
$$\dot{CO_2} = \dot{CO_2}_{in} - \dot{CO_2}_{out}$$
This equation works regardless of the units. By convention n Australia, these quantities are measured in volume of gas (by the ideal gas law we could equally use partial pressures or moles).
Let's tackle the two right hand side quantities one by one.
Carbon dioxide production is denoted \dot{V}_CO2. CO2 is produced when oxygen is consumed to oxidize macronutrients. The ratio of oxygen consumed to CO2 generated is called the respiratory quotient.
$$\dot{CO_2}_{in} = \dot{V}_{CO_2} = RQ \cdot \dot{V}_{O_2}$$
The respiratory quotient depends on the maconutrient. This means it is influenced by diet, and also by some drugs (e.g. carnitine palmitoyltransferase inhibitors like perhexiline, which decreases mitochondrial update of fatty acids, reduced the RQ).
But the big influence here is the rate of oxygen consumption. This is increased any time cellular demands for energy are high, so that is in exercise, sepsis, hyperthyroidism, malignant hypertension, and critical illness in general.
Let's make some assumptions:
Then the partial pressure of CO2 in the alveolus equals the partial pressure of CO2 in the blood.
The ideal gas law tells us that the concentration of CO2 in the alveolar gas is directly proportional to its partial pressure (more molecules = more pressure). Double the pressure, double the molecules.
And clearly, the volume of gas in a breath is proportional to the total amount of CO2. For the same partial pressure, if you double the volume of gas, you double the molecules.
The total amount of CO2 eliminated per unit time is just the amount lost per breath, times breaths per unit time (i.e. resp rate):
$$\dot{CO_2}_{out} \propto RR \cdot V_{alveolar} \cdot \rho_aCO_2$$
The volume of alveolar gas is equal to the tidal volume minus all the bits of the tidal volume that aren't in the alveolus (i.e. are in the airways, or are in non-perfused alveoli). We call this non-participatory fraction dead space:
$$\dot{CO_2}_{out} \propto RR \cdot (V_{tidal} - V_{dead}) \cdot \rho_aCO_2$$
And the product of alveolar volume and resp rate is called alveolar ventilation.
$$\dot{CO_2}_{out} \propto \dot{V}_A \cdot \rho_aCO_2$$
The partial pressure of CO2 is itself directly proportional to the total CO2 content in the blood (dear reader, I leave deriving this from the CO2 equilibrium constant as an exercise, xox). So, with K as our constant of proportionality, we have:
$$\dot{CO_2}_{out} = k \cdot [\dot{V}_A \cdot \rho_aCO_2]$$
And we're done.
All our hard work yields this beauty:
$$\dot{CO_2} = [RQ \cdot \dot{V}_{O_2}] - k \cdot [\dot{V}_A \cdot \rho_aCO_2]$$
Here we have a differential equation of the form:
$$\dot{y} = a - b \cdot y$$
Which we can solve with separation of variables like so:
$$\frac{1}{a - b \cdot y} \frac{dy}{dt} = 1$$
$$\int \frac{1}{a - b \cdot y} dy = \int 1 dt$$
A quick u-substitution yields
$$ - \frac{1}{b} \ln{|a - b \cdot y|} = t + c$$
Being a little naughty and letting our (arbitrary) c absorb the b constant,
$$ \ln{|a - b \cdot y|} = - bt + c$$
$$ y = \frac{a}{b} \pm \frac{e^{c}}{b} e^{-bt}$$
If we only care about the steady state, though, then we can let t trend to infinity and...
$$ y = \frac{a}{b}$$
What did these letters stand for again? Oh yeah,
$$CO_2 = \frac{RQ \cdot \dot{V}_{O_2}}{k \dot{V}_A}$$
Or, for short,
$$CO_2 \propto \frac{\dot{V}_{CO_2}}{\dot{V}_A}$$
This means that total body CO2 is proportional to:
And inversely proportional to:
The neural circuit here is straightforward negative feedback:
Or, to make it even simpler: in health, the lungs can set the CO2 to whatever the brain wants.
The kidneys control pH through three mechanisms:
(a) In the proximal tubule, reabsorbing bicarbonate along with sodium
This occurs due to the activity of carbonic anhydrase in the proximal tubule.
This process continues until no more tubular bicarbonate remains to fuel step (3). The net effect of this is to reabsorb sodium and bicarbonate, without reabsorbing any chloride.
This process is disrupted in proximal RTA, or by a carbonic anhydrase inhibitor
(b) Freely filtering, and actively secreting, phosphates, suphates, and other "titratable acids"
This process is quantitatively unimportant.
(c) Most importantly, generating de novo ammonium and excreting it along with chloride
The process of manufacturing ammonium consumes a hydrogen ion. The net effect is loss of hydrogen and of chloride, without any sodium loss.
This process is disrupted in distal RTA, or in the presence of hyperkalaemia, which competes with ammonium for NKCC2 excretion in the loop of Henle.
All three processes are under direct negative feedback from ECF pH.
The Boston school of thought is derived directly from the Henderson-Hasselbalch equation.
In this paradigm
The main problem is that CO2 also affects the bicarbonate, even without the kidneys doing anything at all (e.g. an increase in CO2 will immediately increase bicarbonate by driving the equilibrium to the right). This means that the bicarbonate is affected by
This system therefore relies on a set of observational rules:
The Copenhagen school of thought tries to isolate the effects of the kidneys and the lungs. It defines two special quantities, called the "base excess" and "standard base excess". In this paradigm
Here's how you make a base excess:
Of course, the blood gas machine uses an algorithm to estimate this quantity.
The standard base excess is a little fancier. The idea is the same, but instead of being concerned with a unit volume of plasma, the quantity concerns a unit volume of ECF. What's the difference? Haemoglobin.
Since haemoglobin is a potent buffer, but is only available to the plasma, the plasma base excess (and indeed bicarbonate) are a biased estimate of the ECF base excess/bicarbonate, which is what we really care about. The standard base excess uses the blood gas analyser's estimate of the Hb to adjust the base excess estimate.
The advantage of this system is that it fully separates the respiratory and metabolic components, such that an acute respiratory disturbance does not affect the SBE. It also reduces cognitive burden because the normal value of the SBE is 0, +/- 3.
Of course, we still need to assess the adequacy of compensation in chronic respiratory disturbances and metabolic disturbances. There's only three rules to know:
In a chronic resp disturbance, the SBE is 0.4 * the change in the PaCO2
In a metabolic alkalosis, the change in CO2 is 0.6 * the SBE
In a metabolic acidosis, the change in CO2 is equal to the SBE
The Stewart approach is a reimaginging of acid-base physiology from first principles of chemistry. It eschews focusing on bicarbonate and hydrogen, as these quantities cannot be directly regulated by the body.
(For example, if a cell pumps out hydrogen ions, then the rate of autoionization of water inside the cell will increase by LCP, driving pH back down to near the previous value; similarly, if the kidneys pump out bicarbonate, this will increase the rate of dissociation of CO2 into bicarbonate).
This all sounds very complicated. Luckily, there are a few independent variables in the system that are no subject to equilibria like this, and Stewart's contention is that these are what is actually regulated by the body (all else is consequent).
In this paradigm:
The best intuition pump for this is to go back to the Henderson-Hasselbalch equation. The pH remains under direct physiological control. But it is the combination of the SID and ATOT that determine the bicarbonate concentration (and therefore the pH).
This is because of electroneutrality. The total amount of anions and cations has to remain constant.
Decreasing the SID adds strong anions (usually chloride or lactate) to the left. Only weak acids, like bicarbonate, can escape to become other compounds, since the strong ions have to remain dissociated. To maintain electroneutrality, bicarbonate is forced into being carbonic acid.
Similarly, changes in the quantities of total acid, e.g. changes in albumin, will change how much conjugate base is competing with bicarbonate for anion-space. This is how a hypoalbuminaemia causes a metabolic alkalosis.
In reality, these factors are not JUST acting on bicarbonate, but on all the weak acids in the body fluids.
This approach does not consider the effect of haemoglobin and also does not consider adequacy of compensation (which is an evolved biological process that cannot be estimated from first principles).
Mid-twenties lost cause.
Trapped in a shrinking cube.
Bounded on the whimsy on the left and analysis on the right.
Bounded by mathematics behind me and medicine in front of me.
Bounded by words above me and raw logic below.
Will be satisfied when I have a fairytale romance, literally save the entire world, and write the perfect koan.