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翻訳と辞書　辞書検索 [ 開発暫定版 ] スポンサード リンク Bicarbonate buffering system ： ウィキペディア英語版 Bicarbonate buffering system The carbon dioxide - carbonic acid equilibrium is catalyzed by the enzyme carbonic anhydrase; the carbonic acid - bicarbonate equilibrium is simple proton dissociation/association and needs no catalyst. Any disturbance of the system will be compensated by a shift in the chemical equilibrium according to Le Chatelier's principle. For example, if one attempted to acidify the blood by dumping in an excess of hydrogen ions (acidemia), some of those hydrogen ions will associate with bicarbonate, forming carbonic acid, resulting in a smaller net increase of acidity than otherwise. This buffering system becomes an even more powerful regulator of acidity when it is coupled with the body's capacity for respiratory compensation, in which breathing is altered to modify the amount of CO2 in circulation. In the above example, increased ventilation would increase the loss of CO2 to the atmosphere, driving the equilibria above to the left. The process could continue until the excess acid is all exhaled. This process is extremely important in the physiology of blood-having animals. It manages the many acid and base imbalances that can be produced by both normal and abnormal physiology. It also affects the handling of carbon dioxide, the constantly produced waste product of cellular respiration. Furthermore, the bicarbonate buffering system plays a vital role in the duodenum, serving to both neutralizegastric acid and stabilize the intracellular pH of duodenalepithelial cells via the secretion of bicarbonate ion. ==Henderson–Hasselbalch equation== A modified version of the Henderson–Hasselbalch equation can be used to relate the pH of blood to constituents of the bicarbonate buffering system:〔(page 556 ), section "Estimating plasma pH" in: 〕 :$pH\; =\; pK\_+\; \backslash log\; \backslash left\; (\; \backslash frac\; \backslash right\; )$ , where: *pKa H2CO3 is the negative logarithm (base 10) of the acid dissociation constant of carbonic acid. It is equal to 6.1. *() is the concentration of bicarbonate in the blood *() is the concentration of carbonic acid in the blood This is useful in arterial blood gas, but these usually state ''pCO2'', that is, the partial pressure of carbon dioxide, rather than H2CO3. However, these are related by the equation:〔 :$()\; =\; k\_\backslash ,\; \backslash times\; pCO\_2$ , where: *() is the concentration of carbonic acid in the blood *''kH CO2'' is a constant including the solubility of carbon dioxide in blood. ''kH CO2'' is approximately 0.03 (mmol/L)/mmHg *''pCO2'' is the partial pressure of carbon dioxide in the blood Taken together, the following equation can be used to relate the pH of blood to the concentration of bicarbonate and the partial pressure of carbon dioxide:〔 :$pH\; =\; 6.1\; +\; \backslash log\; \backslash left\; (\; \backslash frac\; \backslash right\; )$ , where: *pH is the acidity in the blood *() is the concentration of bicarbonate in the blood, in mmol/L *''pCO2'' is the partial pressure of carbon dioxide in the blood, in mmHg 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Bicarbonate buffering system」の詳細全文を読む スポンサード リンク 翻訳と辞書 : 翻訳のためのインターネットリソース Copyright(C) kotoba.ne.jp 1997-2016. All Rights Reserved.