Question

What is the pH of a KOH solution that has [H+] = 1.87 × 10–13 M?

Answer 1

To find the pH of a solution, we have to take the
`-log` of the [H+] of the solution. Essentially you can think that the 'p' means
`-log`.

So to find the pH of this KOH solution, we are going to take the
`-log([H+])` to find the pH.


`pH=-log([H+)]`


`pH=-log(1.87* 10^(-13))`


`pH=2.92* 10^(-4)`

Answer 2

pH = 12.73

Step-by-step explanation:

pH of a solution is defined as the log to base 10 of the hydrogen ion (H+) concentration of the solution.

In the question above,

H+ = 1.87×10⁻¹³M

pH = -log[H+]

pH = -log(1.87×10⁻¹³)

pH = -(-12.73)

pH = 12.73

The pH of a 1.87×10⁻¹³ KOH solution is 12.73