Chloride seems to be the forgotten electrolyte. Nobody cares about it enough to write a physiology book chapter about its secret life. I, for one, would like to see this change. I only hope that one day somebody smarter than me will do it justice with an appropriate erudition.
Total body chloride content
- You have about 45 mmol/Kg of chloride.
- A 70kg male has about 3.2 moles of chloride, or about 115g of chloride
- Of this, 90% is extracellular. Chloride contributes 70% to the total anionic charge of the extracellular fluid.
- The extracellular concentration is about 100mmol/L
It can be said that chloride stalks sodium. Where sodium goes, chloride follows.
Chloride equilibrates easily between the extracellular fluid compartments.
A Gibbs-Donnan effect forces some of it out of the intravascular compartment. Without this, there would be roughly equal concentrations of sodium and chloride: 145mmol each. But: there is enough protein anionic charge in the plasma to repel a significant amount of chloride, and so at equilibrium an extra 5mmol/L or so of chloride hangs out in the interstitial compartment.
Interstitial chloride is slightly higher.
It makes up for the absence of anionic proteins in the interstitial fluid. Some electroneutrality is maintained by a raised chloride, and some by a slightly raised bicarbonate. Overall, there is little difference.
Chloride concentration in the cell is kept low by action of a chloride-potassium co-transporter
There are many of these, and some also co-transport sodium.
It seems most are powered by the concentration gradient of potassium, rather than by ATP.
Surely, sending one's potassium back out of the cell is bad? It doesn't belong out there... Well. There are massively powerful mechanisms in place maintaining the high intracellular concentration of potassium. The potassium extruded with the chloride is rapidly sucked back into the cell by the Na+/K+ ATPase, and the rate of its reuptake far exceeds the rate of chloride removal.
Again, this is one of those situations where the measurements of fluid compartment ion concentrations vary wildly from textbook to textbook. One simply chooses the most believable number.
Total body bicarbonate content
It is difficult to estimate how much bicarbonate one has. The amount of bicarbonate fluctuates, as it is constantly dissociating into carbon dioxide and water; water is massively abundant and carbon dioxide is massively volatile, so the total body bicarbonate relies largely on total body carbon dioxide.
About 70% of carbon dioxide is converted into carbonic acid, of which the bicarbonate ion is the conjugate base.
- One can make guesstimate calculations according to known mmol/L values, in a 70kg person:
- One has 8.4 + 3.15 + 3.15 = 14.7L of interstitial fluid, so that makes 411.6 mmol of HCO3- at 28 mmol/L
- One has 3.15L of intravascular fluid , so that makes 75.6mmol of HCO3- at 24 mmol/L
- One has 21.3 L if intracellular fluid, so that makes 213mmol of HCO3- at 10 mmol/L
- That makes a neat 700.3 mmol of HCO3- in one average 70kg guy.
- A 70kg male has about 700 mmol of free bicarbonate ion, or about 42.7g
- Of this total, about 60% is in the extracellular fluid;
- Of the total, 50% is in the functional ECF.
Bicarbonate equilibrates easily between the extracellular fluid compartments.
A Gibbs-Donnan effect forces some of it out of the intravascular compartment
Bicarbonate is easily converted to CO2 which is highly lipid-soluble, and thus diffuses effortlessly in and out of cells.
Carbonic anhydrase does this reversibly, and at a ridiculous rate. It is probably the fastest-acting enzyme.
Bicarbonate itself finds it difficult to traverse the cell membrane, which to it is essentially impermeable.
Briefly, why all this interest in bicarbonate?
The bicarbonate anion (HCO3-) is a buffer anion, the conjugate anion of carbonic acid (H2CO3 ).
It combines with H+ to form H2CO3 when H+ is in excess, and it dissociates from H+ when H+ is in deficit.
(this is the process of buffering)
It is the H2CO3 form which is metabolized by carbonic anhydrase.
Thus, in the presence of large amounts of H+, lots of H2CO3 is available as a substrate for carbonic anhydrase and this lots of CO2 is formed, in order for you to exhale it.
Total body phosphate content
- You have about 320 mmol/Kg of phosphorus.
- A 70kg male has about 22.5 moles of phosphorus, or about 700 g
- Of this, 85% is bound in the hydroxyapatite matrix of bone.
- That’s 19.1 moles, or 595g. 300 mg of this is exchanged every day as part of normal bone turnover.
- The other 15% is dissolved, and exists largely as the phosphate ion, PO43-
- Say, 14.99% of the remaining 15% is intracellular. That is about 3.4 moles.
- The intracellular concentration is between 60mmol and 100mmol, but only 10mmol are free.
- Phosphate is the most abundant intracellular anion. It acts as an important intracellular buffer.
- The rest is in the extracellular fluid; in total, no more than 12mmol.
- The extracellular concentration is about 1.0mmol/L. This is the only phosphate source to the cells.
- Most of it is present as a univalent species (i.e. with a negative charge of 1). Even though the phosphate ion, when fully ionized, is a trivalent PO43- at physiological pH the divalent PO42- species is the more prevalent (about 80%), and the univalent PO4- species is the other 20%. It takes a pH of 6.8 or so to get to a trivalent majority. This only ever happens intracellularly, where the pH is routinely about 6.9.
Bone phosphate follows the same rules as calcium. It dissolves along with the rest of hydroxyapatite.
Phosphate equilibrates easily between the extracellular fluid compartments.
There really isn’t anything stopping it. It is strongly anionic, so there is slightly more in the interstitial fluid (as it is repelled by the anionic charge of plasma proteins)
Extracellular phosphate behaves in a manner similar to calcium. An authoritative paper by Baker and Worthley on calcium magnesium and phosphate metabolism reports that about 15% of it is bound to protein, another 53% free and ionised, and another 47% compelled with calcium and magnesium.
Phosphate is sucked into the cell by a sodium-phosphate co-transporter, which is more active in the presence of insulin. This process is powered by the awesomely powerful sodium concentration gradient. There are three types (inventively nominated as Type1, 2 and 3); the Type 3 co-transporter seems to be the ubiquitous one, which all of the human cells express.
Total body lactate content
Like bicarbonate, this is one of those things that depends on the nuances of minute-to-minute metabolism. In a normal person, at any given time there may be very little lactate.
Given the below concentrations in mmol/L, and knowing the total body fluid volume of a random 70kg guy, you can estimate that he will have about 22.6 mmol of total extracellular lactate and another 34.5 mmol in his cells
Lactate equilibrates freely across the extracellular fluid
There isn’t enough of it to matter seriously in any of the Gibbs-Donnan effects, or to contribute significantly to the various osmolar forces. Like potassium, it merely exists.
Until your gut becomes ischaemic, and your serum lactate rises to over 20. At this grim stage there is a real and measurable osmolar contribution from the lactate.
Lactate has little trouble getting in and out of cells.
Particularly, muscle cell membranes are highly permeable.
If one wishes to observe lactate more closely, one may visit my brief summary of lactic acidosis.