Sorry, I did make an error when I posted the earlier question:
It should have said:
A solution has [OH-] = 2.0 x 10-^14 M. The [H+] in this solution is?
I hope you can help. Thank you. Sorry about the earlier error.
[H^+](OH^-] = Kw = 1E-14
You have OH^- and Kw, solve for H^+
No problem! I can help you with that. To find the [H+] in a solution given the [OH-], you can use the equation for the ionization constant of water, also known as the Kw.
The Kw is defined as the product of the concentrations of the hydrogen ions ([H+]) and hydroxide ions ([OH-]) in water, and it is equal to 1.0 x 10^(-14) at 25°C.
So, if you have the concentration of hydroxide ions ([OH-]) in the solution, you can use the Kw equation to find the concentration of hydrogen ions ([H+]). The equation is:
Kw = [H+][OH-]
Rearranging the equation to solve for [H+], we get:
[H+] = Kw / [OH-]
Substituting the given value for [OH-] into the equation, we can calculate the [H+].
[H+] = (1.0 x 10^(-14) M) / (2.0 x 10^(-14) M)
[H+] = 0.5
Therefore, the concentration of [H+] in the solution is 0.5 M.