Ionic Product Constant of Water - QS Study
QS Study

H2O and Kc are both constant and combining these constants together make up the ionic product constant for water, written KW.

KW = [H3O+] [OH-]

The value of KW is 1.0 x 10-14 mol2 dm-6 at 25°C. Like any equilibrium constant, KW varies with temperature.

These ions are produced in equal numbers in pure water, so

[H+] = [OH] x 10-14 = [H+]2

[H+] = [OH] = 1.0 x 10-7 Mol.dm-3

Experiments have shown that the value for [H+] x [OH-] always equals 1.0 x 10-14 at 25°C even in solutions (such as acids or bases) where [H+] ≠ [OH-]. This means that if [H+] is known, then [OH-] can be calculated, or vice versa.

Example

Calculate the concentration of OH- ions in 0.10 M HCl

HC1 (aq) → H+ (aq) + Cl- (aq)

HC1 is a strong acid, so [H+ (aq)] will be 0.10 M.

Substituting [H+] = 0.10 into the KW expression, we get:

1.0 x 10-14 = (0.10) x [OH-]

[OH] = 1.0 x 10-13 M