[OH⁻] = 6.31 × 10⁻³ M
Step 1: Calculate pOH as,
pH + pOH = 14
As, pH = 11.8
So,
11.8 + pOH = 14
Or,
pOH = 14 - 11.8
pOH = 2.2
Step 2: Calculate [OH⁻],
pOH is related to [OH⁻] as,
pOH = - log [OH⁻]
Putting value of pOH,
2.2 = -log [OH⁻]
Solving for [OH⁻],
[OH⁻] = 10⁻²'² ∴ 10 = Antilog
[OH⁻] = 6.31 × 10⁻³ M
The concentration of [tex]OH^-[/tex] ions in the solution is 0.0063 M
pH is a quantitative measure of the acidity or basicity of aqueous or other liquid solutions.
pH or pOH is the measure of acidity or alkalinity of a solution.
pOH is calculated by taking negative logarithm of hydroxide ion concentration.
pH = -log [[tex]OH^-[/tex]]
pH + pOH = 14
11.8 + pOH = 14
pOH = 2.2
Putting in the values:
2.2 =-log [[tex]OH^-[/tex]]
[[tex]OH^-[/tex]] =0.0063 M
Hence, the concentration of [tex]OH^-[/tex] ions in the solution is 0.0063 M
Learn more about the pH here:
https://brainly.com/question/16745007
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