Taking into account the definition of pH and pOH, the concentration of H⁺ ions at pH=8 is 1×10⁻⁸ M and the concentration of OH⁻ ions at pH=8 is 1×10⁻⁶ M.
<h3>Definition of pH</h3>
pH is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance.
The pH is defined as the negative base 10 logarithm of the activity of hydrogen ions, that is, the concentration of hydrogen ions or H₃O⁺:
pH= - log [H⁺]= - log [H₃O⁺]
<h3>Definition of pOH</h3>
Similarly, pOH is a measure of hydroxyl ions in a solution and is expressed as the logarithm of the concentration of OH⁻ ions, with the sign changed:
pOH= - log [OH⁻]
<h3 /><h3>Relationship between pH and pOH</h3>
The following relationship can be established between pH and pOH:
pOH + pH= 14
<h3>Concentration of H⁺ ions</h3>
In this case, pH=8. Replacing in the definition of pH:
8= - log [H⁺]
Solving:
<u><em>[H⁺]= 10⁻⁸= 1×10⁻⁸ M</em></u>
Finally, the concentration of H⁺ ions at pH=8 is 1×10⁻⁸ M.
<h3>Concentration of OH⁻ ions</h3>
Being pH= 8, pOH is calculated as:
pOH + 8= 14
pOH= 14 - 8
pOH= 6
Replacing in the definition of pOH the concentration of OH⁻ ions is obtained:
- log [OH⁻]= 6
Solving
<u><em>[OH⁻]= 10⁻⁶= 1×10⁻⁶ M</em></u>
Finally, the concentration of OH⁻ ions at pH=8 is 1×10⁻⁶ M.
Learn more about pH and pOH:
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