Difference between revisions of "PH"
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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). | 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. | + | 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 [[Logarithm|logarithmic]], a change of pH by 1 corresponds to a change in concentration by a factor of 10. |
[[Category:Acid–base chemistry]] | [[Category:Acid–base chemistry]] | ||
Revision as of 05:11, April 18, 2016
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.