We’re being asked to calculate [H_{3}O^{+}] 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 H_{3}O^{+} 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:

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

K_{w} = autoionization constant of water

**K _{w} = 1.0x10**

Calculate [H_{3}O^{+}] and [OH^{−}] for each of the following solutions.

a. pH = 8.57

b. pH = 2.86

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the pH and pOH concept. You can view video lessons to learn pH and pOH. Or if you need more pH and pOH practice, you can also practice pH and pOH practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Driscoll's class at GVSU.