Taking into account the definition of pH and pOH, the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°c is 2.138×10⁻¹⁰ M.
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 hydronium ion H₃O⁺:
pH= - log [H⁺]= - log [H₃O⁺]
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⁻]
The following relationship can be established between pH and pOH:
pOH + pH= 14
Being pOH= 4.33, pH is calculated as:
pH + 4.33= 14
pH= 14 - 4.33
pH= 9.67
Replacing in the definition of pH the concentration of hydronium ions is obtained:
- log [H₃O⁺]= 9.67
Solving:
[H₃O⁺]= 10⁻⁹ ⁶⁷
[H₃O⁺]= 2.138×10⁻¹⁰ M
Finally, the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°c is 2.138×10⁻¹⁰ M.
Learn more about pH and pOH:
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