Buffers blood

The excessive amount of bicarbonate in the blood means that blood has a much greater capacity to neutralize acids. Many acids accumulate in the blood during strenuous activity, for example lactic acid. Excretion of bicarbonate through the kidneys and the removal of carbon dioxide through respiration also regulate the carbonic acid/ bicarbonate blood buffer. 

Probably an example and problems derived from the carbon dioxide-blood buffer system in humans should be in every physical chemistry course. What a rich, complex example this is from Henry s law for the solubility of carbon dioxide in water (blood) to buffer capacity, that is, the rate of change of the law of mass action with proton concentration. The example can be expanded to include nonideal solutions and activities. How many physical chemistry courses use this wonderful and terribly relevant to life example First-year medical students learn this material. 

The membranes of the tubules contain enzyme and active transport systems. One such important enzyme system is carbonic anhydrase, which you might remember as being necessary for establishing the blood-buffer (bicarbonate) system. It performs the same buffering function here allowing... 

Bicarbonate system is still the major blood buffer, however... 

The HCOs/COa system is one of the pvo major blood buffers. Carbonic acid ionizes as a typical weak diprotic acid ... 

Aside from its welhkno vn function as an oxygen carrier, hemoglobin plays an important role as a blood buffer. In order to understand the interrelationship between oxygen uptake and release, and the buffering action of hemoglobin, we must consider the interaction of several simultaneous equilibria, A greatly simplified version of the equilibria is developed below. 

Later, Doisy improved the methods used for the isolation and identification of insulin and contributed to the knowledge of antibiotics, blood buffer systems, and bile acid metabolism. 

The other part of the blood buffer is the hydrogen carbonate ion, HCO3 . If something happens to increase OH in your blood, H2CO3 reacts to lower the OH concentration and keep the pH from increasing. If H+ enters the blood, HCO3 reacts to keep the pH from decreasing. 

The pH of human blood is maintained within a narrow range by a mixture of buffers. The H2CO3/HCO3 system is one of the important parts of the blood buffer. 

You are familiar with the acid-neutralizing abilities of the carbonates and hydrogen carbonates from the discussion about blood buffering and acid rain. Carbonate and hydrogen carbonate antacids react with HCl to form carbonic acid, which decomposes into carbon dioxide gas and water. 

The concentration of H2CO3 in blood is 1/20 of the concentration of HC03 , yet the blood buffer is capable of buffering the pH against bases, as well as against acid. Explain. 

The pH of blood must be measured at body temperature to accurately reflect the status of blood buffers. 

Recall from Chapter 7 that, because the equilibrium constants of the blood buffer systems change with temperature, the pH of blood at the body temperature of 37°C is different than at room temperature. Hence, to obtain meaningful blood pH measurements that can be related to actual physiological conditions, the measurements should be made at 37°C and the samples should not be exposed to the atmosphere. (Also recall that the pH of a neutral aqueous solution at 3TC is 6.80, and so the acidity scale is changed by 0.20 pH unit.)... 

Simple treatment of C02 and 02 dissociation effects action of blood buffers included. 

Complete empirical blood-gas relations including 02 and C02 dissociation effects as well as blood buffering relations. 

When a person exercises, muscle contractions produce lactic acid. Moderate Increases In lactic acid can be handled by the blood buffers without decreasing the pH of blood. However, excessive amounts of lactic acid can overload the blood buffer system, resulting In a lowering of the blood pH. A condition called... 

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