Following this, it is easy and clear to find the end- product of titration. However, the end-point on the titration graph is the same as the maximum point on the first derivative graph. Following this, 19.1mL of Ce4+ in solution forms end-point, which is in red on the table and again represented by a red arrow on the graph 1.Standardization results of titrations are shown in table 4. Primarily, equation (3) was used to calculate the volume end-point. Since the number in the voltmeter did not stabilize as soon as endpoint did pass during titrations. Therefore, because of that, the voltage endpoint was not consistency. Besides voltage is recorded too late on the third titration, and early on the first titration. In addition, there was neglect in the weighing error.Initially, a small amount of Ce4+ is added to the Fe2+ solution, and the number of moles Ce4+ did increase in Fe2+ solution gradually with the continues addition of Ce4+. However, the increase of Ce4+ was persistent until the number of moles of Ce4+ and Fe2+ came to equilibrium. Following this, at the endpoint, the moles of Fe2+ is divided with the Ce4+ solution used and hence the establishment of Ce4+ concentration at the endpoint. Furthermore, mean values of Vceend-point and nFe2+ are used in equation (5). The chemical element of Fe2+.
Work citedKotz, John and Treichel, Paul. Chemistry & Chemical Reactivity. New York: Cengage, 2009.
Please type your essay title, choose your document type, enter your email and we send you essay samples