[betabaggins]

if the Kw at 50 degrees Celsius is 5.0x10^-14 What is the [H+] and [OH-] concentrations?
Would I just take the square root of 5.0x10^-14? Because Kw=[H+][OH-] , so both concentrations would = 2.344228815x10^-7

[Borek]

Square root is a way to go, as stoichiometry of dissociation tells us [H⁺] = [OH^-]. Just remember it is not  2.344228815x10^-7, 2.3×10^-7 at best (Kw doesn't have accuracy high enough to support remaining digits, if you were not taught about error propagation think in terms of significant figures).

[sjb]

I think you're missing a line or two? Do you want to calculate the pH at neutrality, for instance? Also, not sure if sqrt 5 = 2.34...

[Borek]

I think you're missing a line or two? Do you want to calculate the pH at neutrality, for instance?

That was my understanding.

Also, not sure if sqrt 5 = 2.34...

Good point, close, but a bit off.