An Introductory Course of Quantitative Chemical Analysis eBook

This eBook from the Gutenberg Project consists of approximately 220 pages of information about An Introductory Course of Quantitative Chemical Analysis.

In case of need, the ferricyanide can be purified by adding to its solution a little bromine water and recrystallizing the compound.


Procedure.—­Fill one burette with each of the solutions, observing the general procedure with respect to cleaning and rinsing already prescribed.  The bichromate solution is preferably to be placed in a glass-stoppered burette.

Run out from a burette into a beaker of about 300 cc. capacity nearly 40 cc. of the ferrous solution, add 15 cc. of dilute hydrochloric acid (sp. gr. 1.12) and 150 cc. of water and run in the bichromate solution from another burette.  Since both solutions are approximately tenth-normal, 35 cc. of the bichromate solution may be added without testing.  Test at that point by removing a very small drop of the iron solution on the end of a stirring rod, mixing it with a drop of indicator on the tile (Note 1).  If a blue precipitate appears at once, 0.5 cc. of the bichromate solution may be added before testing again.  The stirring rod which has touched the indicator should be dipped in distilled water before returning it to the iron solution.  As soon as the blue appears to be less intense, add the bichromate solution in small portions, finally a single drop at a time, until the point is reached at which no blue color appears after the lapse of thirty seconds from the time of mixing solution and indicator.  At the close of the titration a large drop of the iron solution should be taken for the test.  To determine the end-point beyond any question, as soon as the thirty seconds have elapsed remove another drop of the solution of the same size as that last taken and mix it with the indicator, placing it beside the last previous test.  If this last previous test shows a blue tint in comparison with the fresh mixture, the end-point has not been reached; if no difference can be noted the reaction is complete.  Should the end-point be overstepped, a little more of the ferrous solution may be added and the end-point definitely fixed.

From the volumes of the solutions used, after applying corrections for burette readings, and, if need be, for the temperature of solutions, calculate the value of the ferrous solution in terms of the oxidizing solution.

[Note 1:  The accuracy of the work may be much impaired by the removal of unnecessarily large quantities of solution for the tests.  At the beginning of the titration, while much ferrous iron is still present, the end of the stirring rod need only be moist with the solution; but at the close of the titration drops of considerable size may properly be taken for the final tests.  The stirring rod should be washed to prevent transfer of indicator to the main solution.  This cautious removal of solution does not seriously affect the accuracy of the determination, as it will be noted that the volume of the titrated solution is about 200 cc. and the portions removed are very small.  Moreover, if the procedure is followed as prescribed, the concentration of unoxidized iron decreases very rapidly as the titration is carried out so that when the final tests are made, though large drops may be taken, the amount of ferrous iron is not sufficient to produce any appreciable error in results.

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An Introductory Course of Quantitative Chemical Analysis from Project Gutenberg. Public domain.
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