Conductometric methods:
Straight measurement of conductivity is potentially an extremely sensitive procedure for the determination of various parameters such as the degree of dissociation of a weak electrolytes, dissociation constant, ionic product of water, solubility and solubility product of a sparingly soluble salt.
Based upon the associative change within the conductance/resistance of a solution alongwith the addition of other electrolyte, techniques have been developed for the titration of a strong acid with a strong base, weak acid versus strong base or a weak base and a mixture of a strong acid and weak acid against a strong base. Other categories of titrations that could be performed conductometrically involving displacement titrations: a salt of a weak acid (sodium acetate) versus a strong acid such as HCl or a salt of weak base (ammonium chloride) versus sodium hydroxide; precipitation titrations: silver nitrate versus KCl; complexometric titrations: mercuric nitrate versus KCN or EDTA versus metallic ions and oxidation - reduction (redox) titrations such as the titration of Fe (II) versus KMnO4.
Conductometric methods based upon precipitation or complex formation reactions are not as meaningful as those including neutralization processes. Conductance changes during these titrations are seldom as large as those experiential along with acid-base reactions since no other reagent approaches the great ionic conductance of either hydronium or hydroxide ion.