0.157
<h3>
Further explanation</h3>
Given:
0.348 M of Ba(OH)₂ solution at 25⁰C
Question:
Determine the pOH of Ba(OH)₂.
The Process:
Ba(OH)₂ represents a strong base. The characteristic of a strong base is it has no ionization constant, Kb or the degree of ionization, α. Ba(OH)₂ is fully ionized in water.
The concentration of OH⁻ ions will determine the pOH value and pH by looking at the number of OH⁻ ions or sometimes referred to as base valence.
Let us prepare the concentration of OH⁻ ions.

![\boxed{ \ [OH^-] = \frac{2}{1} \times [Ba(OH)_2] \ }](https://tex.z-dn.net/?f=%5Cboxed%7B%20%5C%20%5BOH%5E-%5D%20%3D%20%5Cfrac%7B2%7D%7B1%7D%20%5Ctimes%20%5BBa%28OH%29_2%5D%20%5C%20%7D)
![\boxed{ \ [OH^-] = 2 \times 0.348 \ M \ }](https://tex.z-dn.net/?f=%5Cboxed%7B%20%5C%20%5BOH%5E-%5D%20%3D%202%20%5Ctimes%200.348%20%5C%20M%20%5C%20%7D)
∴ ![\boxed{ \ [OH^-] = 0.696 \ M \ }](https://tex.z-dn.net/?f=%5Cboxed%7B%20%5C%20%5BOH%5E-%5D%20%3D%200.696%20%5C%20M%20%5C%20%7D)
After obtaining the concentration of OH⁻ ions, we can immediately determine the pOH value.
![\boxed{ \ pOH = -log[OH^-] \ }](https://tex.z-dn.net/?f=%5Cboxed%7B%20%5C%20pOH%20%3D%20-log%5BOH%5E-%5D%20%5C%20%7D)

Thus, we get a pOH of 0.157.
_ _ _ _ _ _ _ _ _ _
What is the pH value of the 0.348 M Ba(OH)₂ solution? Let us continue the rest of the calculation.
Recall that 


∴ 
A pH value closes up to 14 indicates that the solution represents a very strong base. In the same way, if the pH value is very close to one, it means the solution is a very strong acid.
<h3>Learn more</h3>
- What is the molarity of the Ba(OH)₂ solution? (neutralization) brainly.com/question/7882345
- What is the pH of this buffer brainly.com/question/11437567
- Calculate the pH of an acidic buffer system brainly.com/question/9079717