define buffer and write chemical equations for thebicarbonate, phosphate, and protein buffer systems;
define buffer and write chemical equations for the
bicarbonate, phosphate, and protein buffer systems;
We know that The buffer resists the changes of the pH in a solution by converting the strong acid to the weak acid or the strong base to the weak base. Physiological as well as chemical buffer systems regulate the stabilization and control of the body's pH.
The chemical buffer systems (the bicarbonate, the phosphate, and the protein) that neutralize or buffer the excess acid or base in a solution depend on the buffer concentration and working environmental pH. Each chemical buffer system acts best in its optimum pH, and deviation in the environmental pH greatly reduces its effectiveness.
In this reversible reaction, carbonic acid (weak acid) reduces the pH by releasing H ion and bicarbonate ions (a weak base) increase the pH by binding H* ion.
The optimal pH for the bicarbonate buffer system is 6.1. The lungs and kidneys eliminate carbon dioxide (CO₂) constantly.
Mechanism of pH reduction: Excretion of bicarbonate ions (HCO3) by the kidneys reduces the pH, which leads to elevation of Hions in the extracellular fluid. Mechanism of pH raise: Excretion of H and CO, by the kidneys and lungs, respectively, increases the pH.
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