Spectrophotometric Determination of Equilibrium Formal Report
Spectrophotometric Determination of Equilibrium Formal Report
Matt DeLuca
The Department of Chemistry, SUNY College at Brockport
Brockport, NY 14420
CHM 206.04
Abstract:
The main objective of this experiment was incorporating the use of spectrophotometry in an attempt to study the position of equilibrium. Furthermore, after the completion of this experiment, the formation of the equilibrium constant of the iron thiocyanate complex could be determined. In order to accomplish these tasks, five different solutions were made. Upon completion of the experiment, the results of the aforementioned experiments were calculated to an average of the final formation constant of 183.
Introduction:
The experiment for the Spectrophotometric Determination of Equilibrium had the main objectives of determining the position of equilibrium and the formation of the equilibrium constant of the iron thiocyanate complex. In order to do so, the use of a spectrophotometer was incorporated into the experiment. In order to obtain an accurate end result, the absorbance of five various samples was used. In order to determine the formation equilibrium, the constant obtained from Beer’s Law was factored into the calculation. The equation for Beer’s Law is A=bbc. It is important to note that Beer’s Law states that the concentration of a solution is directly proportional to the absorbance. Formally, Beer’s Law relates two factors; the absorption of light, and the properties of the material through which the light is traveling through. Upon further examination of the equation for Beer’s Law, each variable has a corresponding purpose within the overall equation. ‘A’ represents the absorbance of light, and ‘’ is representative of the molar absorptivity. It is also important to note that is highly dependent upon the species measured and its respective wavelength. ‘B’ represents the optical path
Matt DeLuca
The Department of Chemistry, SUNY College at Brockport
Brockport, NY 14420
CHM 206.04
Abstract:
The main objective of this experiment was incorporating the use of spectrophotometry in an attempt to study the position of equilibrium. Furthermore, after the completion of this experiment, the formation of the equilibrium constant of the iron thiocyanate complex could be determined. In order to accomplish these tasks, five different solutions were made. Upon completion of the experiment, the results of the aforementioned experiments were calculated to an average of the final formation constant of 183.
Introduction:
The experiment for the Spectrophotometric Determination of Equilibrium had the main objectives of determining the position of equilibrium and the formation of the equilibrium constant of the iron thiocyanate complex. In order to do so, the use of a spectrophotometer was incorporated into the experiment. In order to obtain an accurate end result, the absorbance of five various samples was used. In order to determine the formation equilibrium, the constant obtained from Beer’s Law was factored into the calculation. The equation for Beer’s Law is A=bbc. It is important to note that Beer’s Law states that the concentration of a solution is directly proportional to the absorbance. Formally, Beer’s Law relates two factors; the absorption of light, and the properties of the material through which the light is traveling through. Upon further examination of the equation for Beer’s Law, each variable has a corresponding purpose within the overall equation. ‘A’ represents the absorbance of light, and ‘’ is representative of the molar absorptivity. It is also important to note that is highly dependent upon the species measured and its respective wavelength. ‘B’ represents the optical path