Buffers: The addition of a little strong acid or base causes a change in the pH of a solution. For example, the addition of one drop of concentrated HCI to a liter of pure water (pH 7) drops the pH of the system from 7 Lo 4 and results in a 1000 fold change in acidity. If such a change occurs in a living system the results are disastrous. Certain combinations of solutes formed by mixing together a weak acid and its conjugate base can prevent large changes in pH when strong bases or acids are added to the system.
The buffers can be prepared by mixing a weak acid with its salt. For example, by mixing acetic acid (CHCOOH) and sodium acetate (CH3COONa). One part of the buffer can neutralize protons (He) and the other part hydroxyl ion (OH). Therefore, these solutions can effectively slow down the rate of pH change.
For example, if an acid, hydrochloric acid (HCI) to an acetic acid-sodium acetate buffer solution, the sodium acetate will react with it and sodium chloride (NaCl) and acetic acid are formed. The acetic acid is a weak acid, therefore releases less H+ ions and result in a slight change in PH. Similarly, if a base, sodium hydroxide (NOH) is added t1 the buffer solution, acetic acids react with it and produce sodium acetate and water. The water ionizes very little and cannot bring profound pH change.
The principal buffer at work inside the cells is the phosphate buffer It consists of pairs of ions, HPO4 – and H2PO4 (the mono hydrogen and dihydrogen phosphate ions).
The dihydrogen phosphate ion (H2P04) is the acid Member of the buffer solution and will neutralize any OH on added to the system by donating a proton (H) to it. The monohydrogen phosphate ion (HPO4) is the conjugate base of the buffer solution and will neutralize any H + added to the system as it is a good proton acceptor.
H2FO4 + OH → HPO4 + H2O
HPO4 + H → H2PO4
Other buffer action mixtures are HCI and Phthalate salts, Boric acid and Sodium hydroxide, Carbonates and Borates, and Potassium dihydrogen phosphate, and Disodium phosphate.
Buffer solutions play significant roles in the normal functioning of living organisms. These are:
The principal buffer ¡n blood ¡s the carbonate buffer. It consists of conjugate pair, carbonic acid, and bicarbonate ion (H2C03 and HC03). Carbonic add neutralize OH– and prevents alkalosis, whereas the bicarbonate neutralizes H+ proton to prevent acidosis.
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