Summarizing pH and pOH

Key Concepts and Summary

The concentration of hydronium ion in a solution of an acid in water is greater than 1.0 \(×\) 10−7M at 25 °C. The concentration of hydroxide ion in a solution of a base in water is greater than 1.0 \(×\) 10−7M at 25 °C. The concentration of \({\text{H}}_{3}{\text{O}}^{\text{+}}\) in a solution can be expressed as the pH of the solution; pH = −log\({\text{H}}_{3}{\text{O}}^{\text{+}}.\) The concentration of OH can be expressed as the pOH of the solution: pOH = −log[OH]. In pure water, pH = 7.00 and pOH = 7.00

Key Equations

  • \(\text{pH}=\text{−log}\left[{\text{H}}_{3}{\text{O}}^{\text{+}}\right]\)
  • pOH = −log[OH]
  • [H3O+] = 10−pH
  • [OH] = 10−pOH
  • pH + pOH = pKw = 14.00 at 25 °C

Glossary

acidic

describes a solution in which [H3O+] > [OH]

basic

describes a solution in which [H3O+] < [OH]

neutral

describes a solution in which [H3O+] = [OH]

pH

logarithmic measure of the concentration of hydronium ions in a solution

pOH

logarithmic measure of the concentration of hydroxide ions in a solution

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