Considering the definition of pH and pOH, you obtain that:
- a solution with a pH = 13 has 0.1 moles of OH⁻ ions per liter.
- a solution with a pH = 13 has 1×10⁻¹³ moles of H⁺ ions per liter.
- a different solution with an H⁺ concentration of 1.0×10⁻⁴ would have a pH= 4.
pH is the Hydrogen Potential. It is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance.
Mathematically, pH is calculated as the negative base 10 logarithm of the activity of hydrogen ions, that is, the concentration of hydrogen ions:
pH= - log [H⁺]
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
In this case, you know that a solution has a pH = 13. So, the pOH can be calculated as:
pOH + 13= 14
pOH= 14 -13
pOH= 1
Then, the concentration of OH⁻ can be calculated as:
1= - log [OH⁻]
[OH⁻]= 10⁻¹
[OH⁻]= 0.1
Finally, a solution with a pH = 13 has 0.1 moles of OH⁻ ions per liter.
On the other side, remembering that pH = 13, the concentration of H⁺ can be calculated as:
13= - log [H⁺]
[H⁺]= 10⁻¹³
[H⁺]= 1×10⁻¹³
So, a solution with a pH = 13 has 1×10⁻¹³ moles of H⁺ ions per liter.
Finally, you have a different solution with an H⁺ concentration of 1.0×10⁻⁴. Replacing in the definition of pH:
pH= - log (1.0×10⁻⁴)
Solving:
pH= 4
Then, a different solution with an H⁺ concentration of 1.0×10⁻⁴ would have a pH= 4.
In summary, you obtain that:
- a solution with a pH = 13 has 0.1 moles of OH⁻ ions per liter.
- a solution with a pH = 13 has 1×10⁻¹³ moles of H⁺ ions per liter.
- a different solution with an H⁺ concentration of 1.0×10⁻⁴ would have a pH= 4.
Learn more:
- brainly.com/question/16032912?referrer=searchResults
- brainly.com/question/13557815?referrer=searchResults
