# PH

(Difference between revisions)
 Revision as of 22:46, 1 December 2011 (view source)← Older edit Revision as of 22:48, 1 December 2011 (view source)Newer edit → Line 1: Line 1: −  The negative [[Logarithm|logarithm]] of the hydrogen ion concentration, the pH, is expressed as follows: + The negative [[Logarithm|logarithm]] of the hydrogen ion concentration, the pH, is expressed as follows: pH = -log10 [H+] pH = -log10 [H+] Line 21: Line 21: Ka= [H+][A-]/[HA] Ka= [H+][A-]/[HA] − Stronger acids will dissociate more and will have a higher Ka value.Elliot WH &amp;amp; Elliot DC, 2009, Biochemistry and Molecular Biology; Oxford + Stronger acids will dissociate more and will have a higher Ka value.Elliot WH &amp;amp;amp; Elliot DC, 2009, Biochemistry and Molecular Biology; Oxford

## Revision as of 22:48, 1 December 2011

The negative logarithm of the hydrogen ion concentration, the pH, is expressed as follows:

pH = -log10 [H+]

The pH scale is a measure of hydrogen ion concentration that eliminates dealing with large powers of 10 and compresses a large range of concentrations onto a more convenient scale, between 1 and 14 as show in the figure below:

### Acid Dissociation

Strong acids are considered to be completely dissociated into ions in dilute solutions. However, weak acids (or bases) are only partially dissociated in solution, and thus an equilibrium is established between the ions and the undissociated molecules.

This equilibrium can be represented by the equation:

[HA]<=>[H+]+[A-].

Where: [HA] is the concentration of undissociated molecules; [H+] is the concentration of hydrogen ions; and [A-] is the concentration of the conjugate base.

This equation can be rearranged to give a Ka value, which is a measure of how strong an acid is.

Ka= [H+][A-]/[HA]

Stronger acids will dissociate more and will have a higher Ka value.

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