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A variety of buffering systems permits blood and other bodily fluids to maintain a narrow pH range, even in the face of perturbations. A buffer is a chemical system that prevents a radical change in fluid pH by dampening the change in hydrogen ion concentrations in the case of excess acid or base.
Various buffer systems exist in body fluids (see Table) to minimise the effects on pH of the addition or removal of acid from them. In ECF, the bicarbonate system is quantitatively the most important for buffering metabolic acids.
Buffers are solutions that contain a weak acid and its a conjugate base; as such, they can absorb excess H + ions or OH – ions, thereby maintaining an overall steady pH in the solution. pH is equal to the negative logarithm of the concentration of H + ions in solution: pH = −log [H +].
12 Σεπ 2022 · Carbonic anhydrase is in red blood cells, renal tubules, gastric mucosa, and pancreatic cells. Other buffer systems in the human body include the phosphate buffer system, proteins, and hemoglobin. All of these contain bases that accept hydrogen ions, which keep the pH from plummeting.
Buffer systems in the body help maintain a narrow pH range, typically between 7.35 and 7.45, which is crucial for cellular function and enzyme activity. The two main buffer systems in the body are the bicarbonate buffer system and the phosphate buffer system.
The body’s acid– base balance is tightly regulated to keep the arterial blood pH between 7.38 and 7.42. Buffer solutions keep the pH constant in a wide variety of chemical actions. A buffer solution is a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid.
