Corrosion Inhibition Theory

Electrochemical metal corrosion reactions are expressed as controlled by anodic reaction,  cathodic reaction, or both. The Tafel slope β is obtained by plotting the log of applied current, i_p versus the reference potential,  η. These slopes can be measured for the cathodic polarisation βc and anodic polarisation  βa :

η = a + b log⁡ i_p

in which, a is an empirical constant; b is the slope
d⁡ η / d⁡ log⁡ i_p = β

When a metal is in corrosion balance with surrounding electrolyte, the anodic currents (i_a) and cathodic currents (i_c) are equal and no net reaction. If the equilibrium is shifted by  whatever reasons, the metal surface will be polarised either cathodically or anodically. For cathodic polarisation, the electrons flow away from metal, i.e. anodic current is evident.  While for anodic polarisation, the electrons push into metal surface.

The corrosion inhibition is to use corrosion inhibitor to influence the corrosion reaction. The free metal corrosion and inhibited metal corrosion reactions are shown in the following Tafel diagram. The point of intersection of anodic reaction and cathodic reaction is the open circuit corrosion potential of the metal in such corroding environment. The corrosion currents are proportional to metal corrosion rate.

The corrosion current can be derived by Stern equation:

in which, I_corr is corrosion current; R is polarisation resistance. Corrosion current, i.e. corrosion rate,  is proportional to inversely of the polarisation resistance.