`pOH = -log([OH^-])`

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pOH^[1] is the measure of basicity of a solution. pOH measurement is derived from the measure of hydroxide ion concentration. Since the ion concentration is small in the solution, it is converted by the equation above to pOH. pH scale ranges from 0 to 14, 0 being acidic and 14 being basic.  At 25^oC the concentration of each ion (H⁺ and OH^-) is 1.0x10^-7(mol/L), when both of the concentrations remain equal then the solution becomes neutral, which is a pH of 7 on the scale.

Description

The equation is 

^[2]

where

• pOH is the basicity measurement (unit-less)
• [OH^-] is the hydroxide ion concentration in units of (mol/L)

Related Material

• pOH from hydronium ion concentration
• pOH from pH
• pH/pOH calculator

Supplement Material

• Khan Academy:
  • Introduction to pH, pOH, and pKw
  • pH, pOH of Strong Acids and Bases

References

[1]https://en.wikipedia.org/wiki/PH#pOH

[2]Whitten, et al. 10th Edition. Pp.713

[pH diagram]http://wiki.chemprime.chemeddl.org/index.php/PH_and_pOH_in_Everyday_Life