| Summary: | This chapter considers buffer solutions, or solutions which show ‘buffer action’ — the ability to oppose changes in pH when small amounts of strong acids and bases are added. An acid buffer solution, one that stabilizes the solution at a pH of less than seven, is typically prepared by making a solution of a weak acid and a salt that supplies its conjugate base. A base buffer, one that stabilizes a solution at a pH of greater than seven, is prepared by making a solution of a weak base and a salt that supplies its conjugate acid. The chapter also studies two buffer systems that help maintain the pH of blood: one arising from a carbonic acid/hydrogencarbonate (bicarbonate) ion equilibrium and another, within red blood cells, involving protonated and deprotonated forms of hemoglobin. It also considers pH regulation by ion transport. The chapter concludes by discussing other buffer systems.
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