6FeSO_{ 4} + K_{ 2}Cr_{ 2}O_{ 7} + 7H_{ 2}SO_{ 4} --> 3Fe_{ 2}(SO_{ 4})_{ 3} + K_{ 2}SO_{ 4} + Cr_{ 2}(SO_{ 4})_{ 3} + 7H_{ 2}O.
If the compounds of iron and chromium, with which alone we are now concerned, be written in such a way as to show the oxides of these elements in each, they would appear as follows: On the left-hand side of the equation 6(FeO.SO_{ 3}) and K_{ 2}O.2CrO_{ 3}; on the right-hand side, 3(Fe_{ 2}O_{ 3}.3SO_{ 3}) and Cr_{ 2}O_{ 3}.3SO_{ 3}. A careful inspection shows that there are three less oxygen atoms associated with chromium atoms on the right-hand side of the equation than on the left-hand, but there are three more oxygen atoms associated with iron atoms on the right than on the left. In other words, a molecule of potassium bichromate has given up three atoms of oxygen for oxidation purposes; i.e., a molecular weight in grams of the bichromate (294.2) will furnish 3 X 16 or 48 grams of oxygen for oxidation purposes. As this 48 grams is six times 8 grams, the basis of the system, the normal solution of potassium bichromate should contain per liter one sixth of 294.2 grams or 49.03 grams.
A further inspection of the dissected compounds above shows that six molecules of FeO.SO_{ 3} were required to react with the three atoms of oxygen from the bichromate. From the two equations
3H_{ 2} + 3O --> 3H_{ 2}O 6(FeO.SO_{ 3}) + 3O --> 3(Fe_{ 2}O_{ 3}.3SO_{ 3})
it is plain that one molecule of ferrous sulphate is equivalent to one atom of hydrogen in reducing power; therefore one molecular weight in grams of ferrous sulphate (151.9) is equivalent to 1 gram of hydrogen. Since the ferrous sulphate crystalline form has the formula FeSO_{ 4}.7H_{ 2}O, a normal reducing solution of this crystalline salt should contain 277.9 grams per liter.
It is possible to purify commercial potassium bichromate by recrystallization from hot water. It must then be dried and cautiously heated to fusion to expel the last traces of moisture, but not sufficiently high to expel any oxygen. The pure salt thus prepared, may be weighed out directly, dissolved, and the solution diluted in a graduated flask to a definite volume. In this case no standardization is made, as the normal value can be calculated directly. It is, however, more generally customary to standardize a solution of the commercial salt by comparison with some substance of definite composition, as described below.