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Arterial blood carbon dioxide tension. P a CO 2 – Partial pressure of carbon dioxide at sea level in arterial blood is between 35 and 45 mmHg (4.7 and 6.0 kPa). [9] Venous blood carbon dioxide tension. P v CO 2 – Partial pressure of carbon dioxide at sea level in venous blood is between 40 and 50 mmHg (5.33 and 6.67 kPa). [9]
6.1 is the acid dissociation constant (pK a) of carbonic acid (H 2 CO 3) at normal body temperature [HCO − 3] is the concentration of bicarbonate in the blood in mEq/L; PaCO 2 is the partial pressure of carbon dioxide in the arterial blood in mmHg; The kidney and the liver are two main organs responsible for the metabolic homeostasis of pH.
The atmospheric pressure is roughly equal to the sum of partial pressures of constituent gases – oxygen, nitrogen, argon, water vapor, carbon dioxide, etc.. In a mixture of gases, each constituent gas has a partial pressure which is the notional pressure of that constituent gas as if it alone occupied the entire volume of the original mixture at the same temperature. [1]
Thus, when O 2 partial pressure is low, hemoglobin-bound O 2 is more readily transferred to myoglobin. Myoglobin, found in high concentrations in muscle tissue, can then transfer the oxygen to muscle tissue muscle fibers , where it will be used in the generation of energy to fuel muscle contraction. [ 3 ]
A blood gas test or blood gas analysis tests blood to measure blood gas tension values and blood pH.It also measures the level and base excess of bicarbonate.The source of the blood is reflected in the name of each test; arterial blood gases come from arteries, venous blood gases come from veins and capillary blood gases come from capillaries. [1]
[4] Hypoxemia is usually defined in terms of reduced partial pressure of oxygen (mm Hg) in arterial blood, but also in terms of reduced content of oxygen (ml oxygen per dl blood) or percentage saturation of hemoglobin (the oxygen-binding protein within red blood cells) with oxygen, which is either found singly or in combination. [2] [5]
Dalton's law (also called Dalton's law of partial pressures) states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. [1] This empirical law was observed by John Dalton in 1801 and published in 1802. [2] Dalton's law is related to the ideal gas laws.
It is a good indicator of respiratory function and the closely related factor of acid–base homeostasis, reflecting the amount of acid in the blood (without lactic acid). Normal values for humans are in the range 35–45 mmHg. Values less than this may indicate hyperventilation and (if blood pH is greater than 7.45) respiratory alkalosis.