Verified Answer :

transitionstate

Answer:

                 [OH⁻]  =  6.31 × 10⁻³ M

SOlution:

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  \(OH^-\) ions in the solution is 0.0063 M

What is pH?

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 [\(OH^-\)]

pH + pOH = 14

11.8 +  pOH = 14

pOH = 2.2

Putting in the values:

2.2 =-log [\(OH^-\)]

[\(OH^-\)] =0.0063 M

Hence, the concentration of  \(OH^-\) ions in the solution is 0.0063 M

Learn more about the pH here:

https://brainly.com/question/16745007

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