What is the [H+] of 1.0 x 10 -12 M OH- solution at 35  °C

To find the [H+] concentration, we first need to know the Kw (ion product of water) at 35 °C. The Kw increases with temperature and at 25 °C it is 1.0 x 10^-14. However, at 35 °C, the Kw is 2.92 x 10^-14.

The relationship between [H+], [OH-], and Kw is given by the equation:

[H+] * [OH-] = Kw

We know the [OH-] is 1.0 x 10^-12 M, so we can substitute this value and the Kw into the equation to solve for [H+]:

[H+] = Kw / [OH-] [H+] = 2.92 x 10^-14 / 1.0 x 10^-12 [H+] = 2.92 x 10^-2 M

So, the [H+] of the solution at 35 °C is 2.92 x 10^-2 M.

To find the [H+] concentration, we first need to know the Kw (ion product of water) at 35 °C. The Kw increases with temperature and at 25 °C it is 1.0 x 10^-14. However, at 35 °C, the Kw is 2.92 x 10^-14.

Given that Kw = [H+][OH-], we can rearrange the equation to find [H+] = Kw / [OH-].

Substituting the given values:

[H+] = (2.92 x 10^-14) / (1.0 x 10^-12)

[H+] = 2.92 x 10^-2 M