Difference between revisions of "PH"

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''For technical reasons this article is titled "PH" The title should be "pH."''
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'''pH''' (potential of Hydrogen) is a measure of the [[acid]]ity or [[base|basicity]] of a [[chemical]] solution.
  
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'''pH''' ('''potential of Hydrogen''') measures the acidity or basicity of a (chemical) solution.  
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pH is defined as the negative log of the [[concentration]] of [[hydrogen]] ions in a solution. (Technically, it is not based on concentration, but ''[[activity]]'', however the activity is very close to the concentration for water solutions).  
  
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Solutions having a pH that is less than 7 are called "acidic".  Solutions having a pH greater than 7 are called "basic".
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Solutions having a pH that is less than 7 are called "acidic".  Solutions having a pH greater than 7 are called "basic". pH equal to 7 is considered to be neutral.  This is the pH of pure water at a temperature of 25 °C. Since pH is logarithmic, a change of  pH by 1 corresponds to a change in concentration by a factor of 10.
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pH equal to 7 is considered to be neutral.  This is the pH of pure water at a temperature of 25 °C.
 
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pH is a logarithmic scale. Roughly, it can be considered to be based on the concentration of protons(H+) in the solution.<ref>Actually, it is based on something called the hydrogen ion ''[[activity]].'' Activity is approximately the same as concentration for dilute solutions in nearly pure water.</ref>  Thus, a change of  pH by 1 corresponds to a change in concentration by a factor of 10. In general, the pH of most substances varies from 0 to 14 although for some extreme cases the pH can be greater than 14 or less than 0.
 
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==Notes and references==
 
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<references/>
 
  
 
[[Category:Chemistry]]
 
[[Category:Chemistry]]

Revision as of 04:17, September 21, 2007

pH (potential of Hydrogen) is a measure of the acidity or basicity of a chemical solution.

pH is defined as the negative log of the concentration of hydrogen ions in a solution. (Technically, it is not based on concentration, but activity, however the activity is very close to the concentration for water solutions).

Solutions having a pH that is less than 7 are called "acidic". Solutions having a pH greater than 7 are called "basic". pH equal to 7 is considered to be neutral. This is the pH of pure water at a temperature of 25 °C. Since pH is logarithmic, a change of pH by 1 corresponds to a change in concentration by a factor of 10.

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