Given KOH solution molarity: 6.8 x 10-4 MCalculate [H+] = ? M (H+ molarity)Group of answer choices6.8 x 10^-107.2 x 10^-41.0 x 10^-141.5 x 10^-11

To calculate the [H+] concentration, we first need to find the [OH-] concentration. Since KOH is a strong base, it will dissociate completely in water to form K+ and OH- ions. Therefore, the [OH-] concentration is the same as the molarity of the KOH solution, which is 6.8 x 10^-4 M.

Next, we use the ion product of water (Kw) to find the [H+]. Kw at 25 degrees Celsius is 1.0 x 10^-14. The relationship between [H+], [OH-], and Kw is given by the equation:

[H+] x [OH-] = Kw

We can rearrange this equation to solve for [H+]:

[H+] = Kw / [OH-]

Substituting the given values:

[H+] = (1.0 x 10^-14) / (6.8 x 10^-4)

Solving this gives [H+] = 1.47 x 10^-11 M.

So, the closest answer choice is 1.5 x 10^-11 M.