Buffer solutions are essential for pH stability, involving weak acids/bases and their conjugates to absorb pH-altering ions. They're crucial in physiological processes like blood pH regulation and are used in various laboratory and industrial applications. The preparation involves precise calculations and standardization to ensure effectiveness in scientific and medical procedures, including specimen preservation.
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Buffer solutions are essential for maintaining pH stability in various environments
Weak Acid and Conjugate Base
Buffer solutions are typically composed of a weak acid and its conjugate base
Weak Base and Conjugate Acid
Buffer solutions can also be composed of a weak base and its conjugate acid
There are two types of buffer solutions: acidic buffers and basic buffers
Buffer solutions stabilize pH by absorbing excess hydrogen ions or hydroxide ions
Acidic buffer systems maintain a pH below 7 by reacting with added acids
Basic buffer systems maintain a pH above 7 by reacting with added bases
pH is a measure of the acidity or alkalinity of a solution
pKa is a measure of the strength of an acid in solution
The Henderson-Hasselbalch equation relates pH, pKa, and the molar concentrations of an acid and its conjugate base to calculate the pH of a buffer solution
Buffer solutions can be prepared by mixing a weak acid with its conjugate base or a weak base with its conjugate acid
The selection of buffer components is based on the desired pH range and the pKa of the components
Buffer solutions are used in various applications, such as titrations and pH measurements in laboratory and medical settings
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In physiological processes, buffers are vital for maintaining blood pH at approximately ______, which is essential for ______ function and enzyme activity.
7.4
cellular
01
Role of Acetate in Acetic Acid Buffer
Acetate reacts with added H+ to form acetic acid, reducing pH change.
02
Acetic Acid Reaction to Strong Base
Acetic acid donates H+ to neutralize OH-, forming water and acetate, stabilizing pH.
