Overview
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1.
To support optimal metabolic activity, the bicarbonate buffer system, an acid-base homeostatic mechanism, balances carbonic acid (H2 CO3), bicarbonate ion (HCO3 -), and carbon dioxide (CO2) in the blood and duodenum, among other organs. Water (H2O) and carbon dioxide (CO2) mix to make carbonic acid (H2 CO3), which quickly dissociates to yield bicarbonate ions (HCO3) and hydrogen ions (H +), as seen in the following reaction:
CO2+H2O = H2CO3 = HCO3 -+ H +
Each buffer system's p H is balanced by the presence of a weak acid (such as H2CO3) and its corresponding base (such as HCO3), which also neutralizes any extra acid or base introduced to the system. When this system isn't functioning correctly, acid-base imbalances, such as acidemia (pH 7.35) and alkalemia (pH > 7.45), happen.
Our bodies must maintain a constant blood pH to operate correctly. The p H of human blood is stabilized by a carbonic acid (H2 CO3) and bicarbonate ion buffer (HCO3 -) H2CO3 plus water results in HCO3 - plus water and a weak acid conjugate base. As an acidic substance enters the circulation, the bicarbonate ions neutralize the hydronium ions, creating carbonic acid and water. The blood's buffering mechanism already includes carbonic acid. Eliminating hydronium ions prevents the blood's p H from becoming acidic.
Equation HCO3 - + H3O += H2CO3 + H20
When a basic substance (more alkaline), such as carbonic acid, enters the circulation, it reacts with the hydroxide ions there to create bicarbonate ions and water. The buffer already has bicarbonate ion concentrations. As a result, the blood's p H is prevented from becoming alkaline by removing the hydroxide ions.
Equation H2CO3 + OH- = HCO3 - + H20
One that completely ionizes in an aqueous solution is a strong acid. When dissolved in water, it constantly loses a proton (H +) (H +). A weak acid is a substance that only slightly ionizes in a solution. A few of its (H +) (H +) atoms are released when it dissolves in water.
2.
By preserving a balance between acid and base, the blood hydrogen carbonate buffer system aids in controlling the pH of the blood. Hydrogen ions (H+) are introduced to the system as blood acidity increases, where they combine with hydrogen carbonate ions (HCO3-) to generate carbonic acid (H2CO3). As a result of this process, the blood's acidity is reduced by removing extra hydrogen ions. H+ + HCO3- -> H2CO3
When the blood is more alkaline, the system operates oppositely. By combining with carbonic acid to generate hydrogen carbonate ions, hydrogen ions are expelled from the system, raising the pH of the blood. H2CO3 -> H+ + HCO3-
Strong acids dissociate and release all of their hydrogen ions when they are in the water. Nitric acid, sulfuric acid, and hydrochloric acid (HCl, H2SO4) are examples of strong acids (HNO3). Weak acids do break down in the water, releasing some hydrogen ions, but only partially. Acetic acid (CH3COOH), citric acid (C6H8O7), and carbonic acid are examples of weak acids (H2CO3). A few examples of therapeutic uses for solid acids also include the production of explosives and colors, and the synthesis of fertilizers and detergents with sulfuric and hydrochloric acids, which aid digestion. Weak acids are often used as food preservatives, taste enhancers, and active medicinal ingredients.
A couple of Equations for dissociation in water: Hydrochloric acid: HCl —> H+ + Cl- and Sulfuric acid: H2SO4 —> 2H+ + SO42-