# Problem: Calculate [H3O+] and [OH−] for each of the following solutions.a. pH = 8.57 b. pH = 2.86

###### FREE Expert Solution

We’re being asked to calculate [H3O+] and [OH] for each of the following solutions.

a. pH = 8.57
b. pH = 2.86

When pH or pOH are given:

The H+ or H3O+ concentration can be calculated from pH using the following equation:

$\overline{)\left[{\mathbf{H}}^{\mathbf{+}}\right]{\mathbf{=}}{\mathbf{10}}^{\mathbf{-}\mathbf{pH}}}$

The OH- concentration can be calculated from pOH using the following equation:

$\overline{)\left[{\mathbf{OH}}^{\mathbf{-}}\right]{\mathbf{=}}{{\mathbf{10}}}^{\mathbf{-}\mathbf{pOH}}}$

The relationship between [H+] and [OH-] is connected by the following equation:

$\overline{){{\mathbf{K}}}_{{\mathbf{w}}}{\mathbf{=}}\left[{\mathbf{H}}^{\mathbf{+}}\right]\left[{\mathbf{OH}}^{\mathbf{-}}\right]}$

Kw = autoionization constant of water

Kw = 1.0x10-14 at T = 25°C

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###### Problem Details

Calculate [H3O+] and [OH] for each of the following solutions.

a. pH = 8.57
b. pH = 2.86