The **pH and pOH **of a compound determine its acidity and basicity.

• **pH**

▪ pH stands for the negative logarithmic function of hydronium ion concentration**▪** can be calculated using the following equation:

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

Take note that: **[H ^{+}] = [H_{3}O^{+}]**

• **pOH**

▪ pOH stands for the negative logarithmic function of hydroxide concentration**▪** can be calculated using the following equation:

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

• The relationship between **pH and pOH** is connected by the following equation:

$\overline{){\mathbf{pH}}{\mathbf{+}}{\mathbf{pOH}}{\mathbf{=}}{\mathbf{14}}}$

On the other hand, if the **pH and pOH are given**:

• The **H ^{+} or H_{3}O^{+} concentration** can be calculated using the following equation:

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

• The **OH ^{-} concentration** can be calculated 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**

Complete this table of values for four aqueous solutions at 25 °C.

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