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

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:

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

Take note that:         [H⁺] = [H₃O⁺]

• pOH

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

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

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

$\boxed{\mathbf{pH}\mathbf{+}\mathbf{pOH}\mathbf{=}\mathbf{14}}$

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

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

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

• The OH^- concentration can be calculated using the following equation:

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

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

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

K_w = autoionization constant of water

K_w = 1.0x10^-14 at T = 25°C