for the remaining chloride of lead was unchanged.  So also, when in a metallic solution one volume of oxygen, or a secondary compound containing that proportion, appeared at the anode, no doubt could arise that hydrogen, equivalent to two volumes, had been determined to the cathode, although, by a secondary action, it had been employed in reducing oxides of lead, copper, or other metals, to the metallic state.  In this manner, then, we learn from the experiments already described in these Researches, that chlorine, iodine, bromine, fluorine, calcium, potassium, strontium, magnesium, manganese, &c., are ions and that their electro-chemical equivalents are the same as their ordinary chemical equivalents.

840.  Propositions iv. and v. extend our means of gaining information.  For if a body of known chemical composition is found to be decomposable, and the nature of the substance evolved as a primary or even a secondary result (743. 777.) at one of the electrodes, be ascertained, the electro-chemical equivalent of that body may be deduced from the known constant composition of the substance evolved.  Thus, when fused protiodide of tin is decomposed by the voltaic current (804.), the conclusion may be drawn, that both the iodine and tin are ions, and that the proportions in which they combine in the fused compound express their electro-chemical equivalents.  Again, with respect to the fused iodide of potassium (805.), it is an electrolyte; and the chemical equivalents will also be the electro-chemical equivalents.

841.  If proposition viii. sustain extensive experimental investigation, then it will not only help to confirm the results obtained by the use of the other propositions, but will give abundant original information of its own.

842.  In many instances, the secondary results obtained by the action of the evolved ion on the substances present in the surrounding liquid or solution, will give the electro-chemical equivalent.  Thus, in the solution of acetate of lead, and, as far as I have gone, in other proto-salts subjected to the reducing action of the nascent hydrogen at the cathode, the metal precipitated has been in the same quantity as if it had been a primary product, (provided no free hydrogen escaped there,) and therefore gave accurately the number representing its electro-chemical equivalent.

843.  Upon this principle it is that secondary results may occasionally be used as measurers of the volta-electric current (706. 740.); but there are not many metallic solutions that answer this purpose well:  for unless the metal is easily precipitated, hydrogen will be evolved at the cathode and vitiate the result.  If a soluble peroxide is formed at the anode, or if the precipitated metal crystallize across the solution and touch the positive electrode, similar vitiated results are obtained.  I expect to find in some salts, as the acetates of mercury and zinc, solutions favourable for this use.