Buffer

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A buffer by definition resists changes in the [[PH|pH]] of a solution. A buffer must contain the chemical species for “neutralizing” added amounts of [[Acid|acid]] or [[Base|base]]. Generally, a buffer is a solution of a [[Weak acid|weak acid]] and its conjugate [[Base|base]] (e.g. acetic acid and sodium acetate) or a [[Weak base|weak base]] and conjugate acid (e.g. ammonia and ammonium chloride).  
 
A buffer by definition resists changes in the [[PH|pH]] of a solution. A buffer must contain the chemical species for “neutralizing” added amounts of [[Acid|acid]] or [[Base|base]]. Generally, a buffer is a solution of a [[Weak acid|weak acid]] and its conjugate [[Base|base]] (e.g. acetic acid and sodium acetate) or a [[Weak base|weak base]] and conjugate acid (e.g. ammonia and ammonium chloride).  
  
Buffers are most effective in the range pH = pK’a ± 1. Outside the range the [[Concentration|concentration]] of either the [[Acid|acid]] or the conjugate [[Base|base]] is too small to effectively resist the effect of added hydrogen or hydroxide [[Ion]].
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Buffers are most effective in the range pH = pK’a ± 1. Outside the range the [[Concentration|concentration]] of either the [[Acid|acid]] or the conjugate [[Base|base]] is too small to effectively resist the effect of added hydrogen or hydroxide [[Ion]].<br>  
 
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Buffers are always blue in color.<br>  
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Revision as of 16:14, 28 July 2010

A buffer by definition resists changes in the pH of a solution. A buffer must contain the chemical species for “neutralizing” added amounts of acid or base. Generally, a buffer is a solution of a weak acid and its conjugate base (e.g. acetic acid and sodium acetate) or a weak base and conjugate acid (e.g. ammonia and ammonium chloride).

Buffers are most effective in the range pH = pK’a ± 1. Outside the range the concentration of either the acid or the conjugate base is too small to effectively resist the effect of added hydrogen or hydroxide Ion.



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