Achieve week 10 #5

[Brenda Tran 3C]

Hi! I am having trouble with this question:
Determine the [H+] , [OH−] , and pOH of a solution with a pH of 13.46 at 25 °C.

I determined pOH and read other posts on how to find [H+] and [OH-] where it's just 10^-pH or 10^-pOH. So correct me if I'm wrong but would the answer be
[H+] = 10^-13.46
[OH-] = 10^-0.54?

I think it's wrong because it won't let me submit the answers so is there another way to solve this?

[Emily2J]

You are given the [H+], so to find [HO-], pH, and pOH, start by finding the pH.
use pH=-log[H+]
then pOH= 14-pH
lastly [OH-]= 10^(-pOH)

[Chem_Mod]

[H+] = 10^-13.46 = 3.467^-14 M
[OH-] = 10^-0.54 = 0.2884 M

[Reagan Feldman 1D]

Here are some equations that can be rearranged in order to help you solve for the pH, [OH-], [H+], or pOH:
pH= -log[H+]
pOH= 14-pH
[OH-]= 10^(-pOH)
1.0 x 10^-14= [H+][OH-]
pOH= -log[H+]