Acid-Base Homeostasis



Acid-Base Homeostasis




HYDROGEN IONS AND pH


Free Hydrogen Ions


Clinical Significance


The free hydrogen ion concentration [H+] in the blood must be maintained within very narrow limits to maintain life. Seemingly slight alterations in the free [H+] may have profound, life-threatening effects on the chemistry of the body. This unusual degree of reactivity is probably related to the small size of the H+ that affords it reaction sites unapproachable by larger ions.



Description


Only hydrogen in free ionic form, however, possesses this chemical potential and is part of the measurement of free hydrogen ion concentration. Hydrogen in chemical combination with other elements (e.g., H2O, HCO3) is not part of the free [H+].


Technically, however, in an aqueous solution, even “free” hydrogen ions are combined chemically with water to form hydronium ions (e.g., H3O+, H5O+). Nevertheless, the distinction between free hydrogen ions and hydronium ions is not important for clinical purposes.


Sometimes, a comparison is also made between H+ activity and H+ concentration. Most hydrogen ion analyzers measure activity rather than actual concentration. Here again, however, there is little clinical significance to this differentiation. Thus, the term hydrogen ion concentration is used to refer to hydrogen ion measurements throughout this text.



pH


Definition


The actual [H+] in the blood is very low, approximately 0.00000004 equivalents per liter (Eq/L). Obviously, monitoring clinical changes using these units would be a very difficult and cumbersome process. Therefore, it has become customary to express [H+] as pH. The definition of pH is the negative log of the free [H+]. Although this definition appears to be complex, pH is a less cumbersome method of assessing the amount of H+ present in a given fluid. The normal range for pH in arterial blood is 7.35 to 7.45.




Acid-Base Balance


Acids


Free hydrogen ions enter the blood on their release from other chemical substances. Any chemical substance capable of releasing a H+ into solution is defined as an acid. Therefore, the greater the number and quantity of acids present in solution, the higher the [H+] (and lower the pH) will be. A variety of acids are normally present in the blood, and these acids serve as the source of free hydrogen ions.




pH Homeostasis


Human cells and organs function best under constant internal conditions including normal pH. Maintenance of a constant internal environment is called homeostasis. Both acids and bases must be regulated closely to ensure stable levels and a normal pH. Maintenance of a constant pH may be called pH homeostasis.


The dynamic regulation of blood pH is accomplished through the interaction of the lungs, the kidneys, and the blood buffers. The lungs and kidneys precisely maintain levels of acids and bases present in the blood. The blood buffers serve primarily a protective role, preventing large changes in pH when abnormal conditions expose the blood to acid-base abnormalities.



Acid Homeostasis


Normal body metabolism tends to result in an accumulation of excess acid. Thus, it is important that the body excrete acid at a rate equivalent to its production to maintain pH homeostasis.






THE LUNGS AND REGULATION OF VOLATILE ACID


Underlying Chemistry


The role of the lungs in human acid-base balance and pH homeostasis is to maintain the concentration of carbonic acid [H2CO3] at constant levels in the arterial blood. As described earlier, the lungs are the major organs of volatile acid (i.e., H2CO3) excretion. Therefore, it is the exclusive responsibility of the respiratory system to excrete carbonic acid in quantities that are exactly in proportion to its production.


Some fundamental principles and chemical relationships must be grasped to fully understand the mechanisms involved in H2CO3 homeostasis. These basic chemical relationships and principles include chemical equilibrium, the law of mass action, the hydrolysis reaction, and the direct, linear relationship between dissolved CO2 and H2CO3.



Chemical Equilibrium


A reversible chemical reaction can proceed in either direction. In reversible chemical reactions, chemical equilibrium exists when the rate of the reaction in one direction is equal to the rate of the reaction in the opposing direction. Chemical equilibrium does not mean that the concentrations of constituents on both sides of an equation are equal.


A closed chemical system is one in which all the reactants and products in a chemical reaction must remain within that system. Once chemical equilibrium for a particular reaction is reached in a closed system, the concentrations of the various constituents do not change. The reaction continues to proceed in both directions but a state of dynamic equilibrium is maintained.


When the concentration of the substances on the left side of a chemical reaction at equilibrium is greater than the concentration of the constituents on the right side, the reaction is said to be shifted to the left. For example, the equation shown in Equation 8-1 is said to be shifted to the left because the concentration of reactants on the left is greater than the concentration of H2CO3. Nevertheless, the reaction is still at equilibrium. Also note that the arrow pointing to the left is longer than the arrow pointing to the right. This designation shows that the reaction is shifted to the left at equilibrium.


H2O+CO2H2CO3(340)+(340)(1) Equation 8-1


image Equation 8-1



Law of Mass Action


Once achieved, a reaction remains at equilibrium in a closed system. If an additional amount of one of the constituents is added to the closed system from an external source, however, a new equilibrium is established. This new equilibrium partially counteracts the initial imbalance in the equilibrium caused by the constituent that has been added. The change in equilibrium in response to a change in the amount of one of the reaction constituents is referred to as the law of mass action.


Thus, if there is an increase in one of the reactants on the right side of the equation, the law of mass action causes the equilibrium point to shift to the left to partially counteract the disturbance. For example, in Equation 8-1, if 5 units of external H2CO3 were added to this equilibrium in a closed system, the equilibrium would shift to the left to partially counteract the alteration. The change in units shown in Equation 8-2 shows the direction of changes that would occur in response to the additional H2CO3 in the system. Conceptually, the increase in mass on the right side of the equation pushes the reaction to the left side of the equation.


H2O+CO2H2CO3(343)+(343)(3) Equation 8-2


image Equation 8-2


A similar phenomenon occurs if one of the constituents is removed from the closed system. In this case, however, the change in equilibrium is an attempt to restore the lost constituent. If CO2 is removed from Equation 8-2, the equilibrium would shift slightly to the left to attempt to restore the lost CO2. The change in units in Equation 8-3 shows the general direction of changes that would accompany the loss of CO2. Note that the removal of CO2 from the system leads to a fall in H2CO3 concentration due to the law of mass action.


H2O+CO2H2CO3(344)+(340)(2) Equation 8-3


image Equation 8-3



Hydrolysis Reaction


CO2 is produced continuously in the cells of the body as an end product of aerobic metabolism. This CO2 then diffuses to the systemic circulation where some of it reacts with water to form carbonic acid. This reaction, shown in Equation 8-4, is called the hydrolysis reaction because water (hydro) is broken down (lysed) as it reacts with dissolved CO2 to form carbonic acid. Because all acids are capable of releasing hydrogen ions, the release of free H+ from carbonic acid is also shown in Equation 8-4.


H2O+CO2H2CO3HCO3+H+ Equation 8-4


image Equation 8-4



Direct Relationship between [CO2] and [H2CO3]


Because of their common involvement in the hydrolysis reaction, there is a direct, linear relationship between the concentration of dissolved CO2 and the concentration of carbonic acid [H2CO3] in the blood. At 37° C, each H2CO3 molecule in solution is in equilibrium with approximately 340 CO2 molecules, as shown in Equation 8-1.364 Earlier estimates reported that the ratio was greater than 700 to 1; however, improved methods suggest the ratio given here. When blood PCO2 levels increase, blood levels of H2CO3 likewise increase. Thus, PCO2 can be used as a marker of blood volatile acid (i.e., H2CO3) levels.



Carbonic Acid Production

Based on the law of mass action, the CO2 that builds up at the tissues leads to a parallel increase in carbonic acid and ultimately hydrogen ions (Fig. 8-1). Thus, there is an increase in the amount of carbonic acid present in the blood as it passes the tissues and CO2 enters. Venous blood has more CO2 and carbonic acid than arterial blood. In fact, that is why venous blood is slightly more acidic (pH = 7.38) compared with arterial blood (pH = 7.40). Actually, the difference in pH would be more substantial were it not for the many effective buffer systems in the blood.




Carbonic Acid Excretion

When the venous blood reaches the lungs, the increased CO2 and carbonic acid that entered the blood at the tissues must be excreted. This is precisely the role of the lungs in acid-base balance: to excrete CO2 and carbonic acid at the same rate that it is being produced. Figure 8-2 shows that as CO2 diffuses into the alveoli, the law of mass action forces the hydrolysis reaction to the left. The net effect of this action is a reduction in carbonic acid and a decrease in the number of hydrogen ions in the blood. Thus, as CO2 is excreted via the lungs, the body is functionally excreting H2CO3.




CO2 Homeostasis


It has been shown that carbonic acid levels in the blood closely parallel dissolved CO2 levels. Dissolved CO2 is maintained at constant internal levels both because of its direct effect on pH and for other physiologic reasons. The maintenance of constant arterial blood PCO2 levels can also be called CO2 homeostasis.The physiologic and metabolic processes that ultimately determine blood CO2 levels are explored.


The arterial PCO2 at any given moment depends on the quantity of CO2 entering the blood from the tissues and the quantity of CO2 leaving the blood via the lungs. The amount of CO2 entering the blood, in turn, depends on the metabolic rate and the substrate being metabolized. The volume of CO2 produced per minute (i.e., CO2 production) is designated as the imageCO2.


Excretion of CO2, on the other hand, depends on alveolar ventilation.Alveolar minute ventilation is the amount of fresh gas that reaches functional (i.e., perfused) alveoli each minute. The symbol for alveolar ventilation per minute is imageA. The balance of imageCO2 and imageA determines the arterial PaCO2 at any given instant, which is shown in Proportion 8-1.


CO2 HOMEOSTASISV˙CO2V˙A=PaCO2 Proportion 8-1


image Proportion 8-1



CO2Production


CO2 production depends on both the quantity and the nature of metabolism. The quantity of metabolism varies directly with body temperature. Metabolism increases as an individual’s body temperature increases. The nature of metabolism depends on the type of foodstuff (e.g., fat, protein, carbohydrate) being metabolized. For example, carbohydrate metabolism produces more CO2 than does fat metabolism.


In normal humans, increases in CO2 production, such as during exercise, are balanced physiologically by increasing alveolar ventilation proportionately. Sometimes, however, increases in CO2 production cannot be offset by increased ventilation. This finding may occur when CO2 production is high (e.g., patients with burns, total parenteral nutrition, sepsis) or when the ventilatory system is compromised.


Large increases in metabolism and CO2 production sufficient to result in PaCO2 elevation may occur occasionally in patients with sepsis (blood infection) or massive burns. Also, an increase in blood PaCO2 can occur after intravenous administration of the drug sodium bicarbonate (NaHCO3) to a patient who is unable to increase alveolar ventilation.365 Because bicarbonate is one of the factors in the hydrolysis reaction, its presence in increased quantities pushes the reaction to the left, which, in turn, has the effect of increasing dissolved CO2 and H2CO3 levels in the blood.


The individual with a normal respiratory system responds to the increased CO2 with a parallel rise in alveolar ventilation and CO2 excretion. The inability to increase alveolar ventilation may be seen, however, when central nervous system ventilatory control mechanisms are not intact or when the respiratory muscles are paralyzed. Paralysis of the ventilatory muscles may occur after trauma or pharmacologic intervention for control of mechanical ventilation. Thus, in these situations the clinician should try to minimize CO2 loading in the blood or to provide the patient with some type of ventilatory support to aid in excretion of the additional CO2 load.



CO2Excretion


In the clinical setting, increased CO2 production is usually balanced by increasing alveolar ventilation. Furthermore, most clinical changes in PaCO2 are a result of changes in alveolar ventilation. Nevertheless, it is becoming increasingly clear that changes in CO2 production can also lead to PaCO2 alterations.


To show the inverse relationship between alveolar ventilation and PaCO2, Proportion 8-1 is sometimes simplified to the form shown in Proportion 8-2. In this proportion, imageCO2 is considered to be a constant and the number one is substituted in the numerator. The proportion becomes simply an inverse relationship between PaCO2 and alveolar ventilation.An increase in alveolar ventilation results in a decreased PaCO2. Conversely, a decrease in alveolar ventilation causes an increased PaCO2.


SIMPLIFIED CO2 HOMEOSTASIS1V˙A=PaCO2 Proportion 8-2


image Proportion 8-2



Minute Ventilation

The amount of gas moving in and out of the lungs with each breath is called the tidal volume (VT). The number of breaths taken each minute is often referred to as the frequency or respiratory rate (RR). Exhaled minute ventilation (imageE) can be calculated as shown in Equation 8-5.


SIMPLIFIED CO2 HOMEOSTASIS1V˙A=PaCO2 Equation 8-5


VT×RR=imageE Equation 8-5


Minute ventilation, however, is not a very reliable index of the adequacy of ventilation. The drawback of minute ventilation is that it does not tell us if the lungs are excreting CO2 in correct proportion to its production. To assess the adequacy of ventilation one must get an arterial blood gas and evaluate the PaCO2. The PaCO2 is the best index available to assess the adequacy of ventilation relative to CO2 production. If the lungs are maintaining CO2 homeostasis, the PaCO2 is maintained within the normal range (i.e., PaCO235 to 45 mm Hg).



Alveolar Ventilation

As shown in Proportion 8-2, PaCO2 is inversely proportional to alveolar ventilation. Alveolar ventilation differs from minute ventilation in that only the gas that reaches functional (i.e., perfused) alveoli is considered alveolar ventilation; in other words, deadspace volume (VD) (see Chapter 6) is subtracted from the tidal volume (VT) to determine alveolar ventilation (imageA). The formula for calculation of alveolar minute ventilation is shown in Equation 8-6.


SIMPLIFIED CO2 HOMEOSTASIS1V˙A=PaCO2 Equation 8-6


imageA=(VT-VD)×RR Equation 8-6


One can readily see that any increase in tidal volume or RR (or a decrease in deadspace) increases alveolar ventilation, assuming of course that all other variables remain constant. An increase in alveolar ventilation, in turn, lowers PaCO2. Conversely, a fall in RR or tidal volume (or an increase in deadspace) decreases alveolar ventilation and increases PaCO2. When a change in PaCO2 is seen clinically, Equation 8-6 should be analyzed to determine what variable has resulted in the change in the patient’s ability to excrete CO2.



Minute Ventilation versus Alveolar Ventilation

Table 8-1 shows three sets of parameters where the minute ventilation is the same (6000 mL/min); however, alveolar ventilation and CO2 excretion are grossly different.Figure 8-3 similarly illustrates how alveolar ventilation and deadspace ventilation would be impacted by the breathing patterns inTable 8-1. During normal breathing (seeFig. 8-3,A), most ventilation is effective alveolar ventilation. If minute volume remains constant, alveolar ventilation will increase with larger tidal volumes and a slower respiratory rate (seeFig. 8-3,B). Finally, if breathing is very rapid and shallow, deadspace ventilation can actually exceed alveolar ventilation (seeFig. 8-3,C) despite a constant minute ventilation.





Note likewise that the PaCO2 varies inversely with the alveolar ventilation. The inadequacy of minute ventilation as an index of the adequacy of ventilation is clearly shown in Table 8-1 and Figure 8-3. The PaCO2 is the only reliable index of the adequacy of ventilation.


It should also be noted that inTable 8-1 and Figure 8-3, deadspace is considered a constant 150 mL/breath. In these sets, changes in alveolar ventilation are due to alterations in VT and RR. In many disease states, deadspace varies considerably from this value. Thus, even when tidal volume and RR are known, the blood gas and specifically the PaCO2 are necessary to assess the adequacy of imageA and the ability of the body to maintain CO2 homeostasis.



CO2Transport


CO2 is transported in the blood in both the plasma and within the red blood cells (erythrocytes). The mechanisms by which CO2 is actually carried in these two compartments are reviewed. The transport of CO2 in the blood is related intimately to acid-base status and homeostasis. CO2 is carried in the blood in four basic forms: dissolved CO2, carbonic acid (H2CO3), bicarbonate (HCO3), and carbamino compounds.



Dissolved CO2


As described in Chapter 3, gases dissolve in liquids in direct proportion to their partial pressures. Furthermore, the volume of gas dissolved in a given liquid depends on the solubility coefficient of that gas in that particular fluid. The solubility coefficient of CO2 in blood is approximately 0.072 vol%/mm Hg, which, of course, is much higher than the solubility coefficient of O2(0.003 vol%/mm Hg). Given a normal PaCO2 of 40 mm Hg, the normal volume of dissolved CO2 in the arterial blood is approximately 2.9 vol%.


In comparison with O2, however, CO2 is sometimes reported in units of mEq/L. The solubility coefficient of CO2 in units of mEq/L is 0.03 mEq/L/mm Hg. Thus, given a normal arterial PCO2 of 40 mm Hg, the normal volume of dissolved CO2 in the plasma is (40 mm Hg × 0.03 mEq/L/mm Hg) 1.2 mEq/L. Dissolved CO2 transport accounts for only approximately 8% of the total volume of CO2 transported from the tissues to the lungs. The factor for converting CO2 in vol% to mEq/L is (vol%/2.23 = mEq/L).



Carbonic Acid


As shown previously in Equation 8-1, the concentration of carbonic acid [H2CO3] in the blood varies directly with the quantity of dissolved CO2, because these two substances are related directly via the hydrolysis reaction. The amount of actual H2CO3 in the blood, however, is minute (0.006%) in comparison with total CO2 transport.


The reason for this unbalanced relationship is that the chemical equilibrium point of the reaction is such that the ratio of dissolved [CO2] to [H2CO3] is approximately 340 to 1 (see Equation 8-1).364 In other words, the reaction is shifted far to the left. Thus, although the quantitative relationship between dissolved CO2 and H2CO3 is very important from an acid-base perspective, the volume of CO2 being transported in the form of H2CO3 is negligible.


In some texts, H2CO3 is excluded as a mechanism of CO2 transport because of its nominal role. Nevertheless, it is included here for completeness and to reinforce understanding of the direct relationship between the quantities of dissolved CO2 and H2CO3.

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Jul 10, 2016 | Posted by in RESPIRATORY | Comments Off on Acid-Base Homeostasis

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