Question

What is the pH of a solution with a [OH–] of 4.1 × 10–3 M?What is the pH of a solution that has [H3O+] = 6.0 × 10−3 M?

Answer 1

pH = 11.61

Explanations:

The formula for calculating the pOH of a solution is expressed as:

`pOH=-log[OH^-]`

Given the following parameters

`[OH^-]=4.1*10^(-3)M`

Substitute

`\begin{gathered} pOH=-log(4.1*10^(-3)) \\ pOH=-(-2.39) \\ pOH=2.39 \end{gathered}`

Determine the pH of the solution

`\begin{gathered} pH+pOH=14 \\ pH=14-pOH \\ pH=14-2.39 \\ pH=11.61 \end{gathered}`

Hence the pH of the solution is 11.61