Rules:

The subsequent approximate rules will be found useful.

• The smaller the conductivity of the ion that replaces the reacting ion, the more accurate will be the result. Therefore it is preferable to titrate a silver salt along with lithium chloride rather than with HCl. Commonly, cations should be titrated along with lithium salts and anions within acetates as these ions have low conductivity.
• The larger the conductivity of the anion of the reagent that reacts with the cation to be determined or vice versa, the more acute is an angle of titration curve.
• The titration of a slightly ionized salt does not provide good results, because the conductivity increases constantly from the commencement. Therefore, the salt present in the cell should be virtually fully dissociated; for a same purpose; the added reagent should also be as strong electrolyte.
• Throughout a titration the volume of the solution is always increasing, unless the conductance is corrected for this effect, non linear titration curves result. The correction could be accomplished through multiplying the observed conductance either through total volume (V+V´) or through the factor (V+ V´)/V, whereas V is the initial volume of solution and V´ is the total volume of the reagent added. The correction presupposes in which the conductivity is a linear function of dilution; this is true only to a first approximation.
• Within the interest of keeping V small, an reagent for the conductometric titration is ordinarily several times more concentrated than the solution being titrated (at least 10-20 times). A micro burette might then be used for the volumetric measurement.