Calculate the hydrogen-ion concentration (H+] for the aqueous solution in which [OH-1 is 1 x 10-12 mol/L.

[H+] = 0.01mol/L

Explanation:

p[OH] = - log[OH-]

[OH-] = 1*10^-12

pOH = - Log[1*10^-12]

pOH = 12.

But pH + pOH = 14

pH = 14 - pOH

pH = 14 - 12

pH = 2

pH = - Log[H+]

2 = - Log[H+]

Take the anti log of both sides

10⁻² = [H+]

[H+] = 0.01

The hydrogen ion concentration is 0.01mol/L

Answer:If we have [H+][OH-] = Kw = 1.0 x 10^-14

Then [H+] = Kw / [OH-] = 1.0x 10^-14 / 1 x 10^-11 = 1 x 10^-3 mol/L

And here is the solution - as you can see it is an acidic one:

pH = - log [H+] = - log 1 x 10^-3 = 3 < 7