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Buffers play a crucial role in stabilizing the pH of a solution by mitigating the effects of small amounts of added acid or base. They consist of a weak acid and its conjugate base or a weak base and its conjugate acid. A solution of acetic acid and sodium acetate is an example of a buffer that consists of a weak acid and its salt: CH3COOH (aq) + CH3COONa (aq). An example of a buffer that consists of a weak base and its salt is a solution of ammonia and ammonium chloride: NH3 (aq) + NH4Cl (aq).

This combination prevents significant pH changes as long as the buffer's capacity is not exceeded. For example, human blood uses a carbonic acid-bicarbonate buffer system to maintain its pH near 7.4. In a buffer, the weak acid component neutralizes added bases by reacting with hydroxide ions, while the conjugate base neutralizes added acids by reacting with hydronium ions.

Теги
BufferPHWeak AcidConjugate BaseWeak BaseConjugate AcidAcetic AcidSodium AcetateAmmoniaAmmonium ChlorideCarbonic AcidBicarbonateBlood PH

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3.12 : Buffers: Overview

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3.1 : Acid–Base Titration: Overview

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3.2 : Titration of a Strong Acid with a Strong Base

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3.3 : Titration of a Weak Acid with a Strong Base

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3.4 : Titration of a Weak Base with a Strong Acid

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3.5 : Titration of a Weak Acid with a Weak Base

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3.6 : Solution Composition During Acid/Base Titrations

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3.7 : Mixtures of Acids

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3.8 : Titration in Nonaqueous Solvents

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3.9 : Titration of Polyprotic Base with a Strong Acid

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3.10 : Titration of Polyprotic Acids with a Strong Base

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3.11 : Composition of Polyprotic Acid Solutions as a Function of pH

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3.13 : Buffers: Buffer Capacity

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3.14 : Leveling Effect

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