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Buffer Solutions and Their Importance

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Buffer solutions play a critical role in maintaining the pH of blood plasma, ensuring it remains around 7.4 for optimal physiological function. These solutions, consisting of weak acids or bases and their conjugates, resist pH changes by neutralizing added acids or bases. The text delves into buffer range and capacity, the Henderson-Hasselbalch Equation for pH calculation, factors influencing buffer capacity, and the bicarbonate buffer system's role in human blood.

The Role of Buffer Solutions in Blood Plasma

Buffer solutions are vital in maintaining the pH of blood plasma, keeping it consistently near 7.4, which is essential for proper physiological function. These solutions are composed of a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid. They work by neutralizing added acids or bases, thereby resisting changes in pH. The Bronsted-Lowry theory provides a framework for understanding buffers, defining acids as substances that donate protons (hydrogen ions) and bases as those that accept protons. The resulting conjugate acid-base pairs form the backbone of buffer systems.
Laboratory with beaker containing light green liquid, pH meter, three erlenmeyers with colored liquids and box of pipette tips.

Defining Buffer Range and Capacity

The effectiveness of a buffer is described by its buffer range and buffer capacity. The buffer range is the pH interval in which the buffer effectively neutralizes added acids or bases. It is typically within one pH unit above or below the pKa of the weak acid in the buffer. The buffer capacity is the measure of how much acid or base can be added to a buffer solution before its pH changes significantly, usually by one pH unit. It is directly proportional to the concentrations of the acid and base components in the buffer; higher concentrations result in a greater buffer capacity.

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00

According to the ______-______ theory, acids are proton donors and bases are proton acceptors, forming the basis of ______ systems.

Bronsted-Lowry

buffer

01

Buffer Range Definition

pH interval where buffer neutralizes acids/bases, typically ±1 pH unit from pKa.

02

Buffer Capacity Factors

Directly proportional to acid/base concentrations in buffer; higher concentrations, higher capacity.

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