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Determining of the equilibrium constant for the formation of FeSCN2+

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    Introduction

    The aim of this experiment was to find the equilibrium concentration and so find Kc. A dilution computation was formed to find the concentration of SCN- and Fe ( SCN ) 2+. Each cuvette was filled to the same volume and can be seen in table 1. Then the optical densities were recorded from each cuvette and can be seen in tabular array

    A Beer’s jurisprudence secret plan was made from the information that was recorded from the optical optical density. During the 2nd portion of the experiment Fe ( NO3 ) 3 was added and diluted with HNO3. All of the cuvettes were assorted with the same solutions in the 2nd portion of the experiment. which can be seen in table 2. A dilution computation was made to find the initial concentration of Fe3+and SCN- . Then the expression Abs + b/ incline was used to find the equilibrium concentration which lead to the computation of each Kc per test.

    Chemical reaction Fe3+ + SCN- FeSCN2+.

    Decision

    An acid and a base were assorted together throughout the experiment. which resulted in a bright orange color. It was determined that utilizing the tintometer at 565nm the would give the optimal wavelength because it was the closest optical density to 430nm. All of the cuvettes were filled to 3mL so at that place would non be another dependent variable. Whenever Fe3+ would come in contact with SCN- there would be a color alteration. Relatively all of the Kc were close to each other as they should be because the lone variable that affects a alteration Kc and the temperature was kept consent throughout the experiment. The mean Kc from all five tests is 1. 52 ten 10 2.

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