Meeting Time: Absorbance Vs. Concentration
Ahmad Almusa
Signature
Group participants: [List names]
Section Number: [List 3-digit number]
Meeting Time: [Fill in the lab meeting time]
TA: [Fill in the lab TA’s name] INTRODUCTION
In this experiment I calculated the equilibrium constant for the reaction shown below under different conditions to determine if the equilibrium constant is really constant. Fe3+ (aq) + SCN– (aq) ←→ FeSCN2+ (aq)
A big part of this lab includes understanding (and in the end proving) that absorbance is directly proportional to the concentration of a solution (Beer’s Law), and if Absorbance v. Concentration is graphed, a straight line will result. The regression line’s equation is used to determine the concentration of an unknown solution once the percent of T has been measured. The equation of Beer’s Law (A=abc) is an efficient way of …show more content…
Sources of uncertainty: Improper calibration of weighing balance, old chemicals used in the experiment.
CONCLUSION
In this lab, we determined equilibrium constant from the reaction between aqueous iron III nitrate and potassium thiocyanate, which was the purpose of the lab. Though the results were not exactly as expected, the data helped the students compute values that were close to the desired values. The results tended toward the uppers 100’s lower 200’s, which were near what was expected. Overall, the experiment was successfully performed and helped us to familiarize with the lab equipment, as well as learn how to deal with the contingency of the temperature value fluctuating due to environmental influences.
REFERENCES
[1] http://chemwiki.ucdavis.edu/Physical_Chemistry/Spectroscopy/Electronic_Spectroscopy/Electronic_Spectroscopy_Basics/The_Beer-Lambert_Law
[2] Beer.1852. Determination of the absorption of red light in colored liquids. Annalen der Physik und Chemie, vol. 86, pp.
Signature
Group participants: [List names]
Section Number: [List 3-digit number]
Meeting Time: [Fill in the lab meeting time]
TA: [Fill in the lab TA’s name] INTRODUCTION
In this experiment I calculated the equilibrium constant for the reaction shown below under different conditions to determine if the equilibrium constant is really constant. Fe3+ (aq) + SCN– (aq) ←→ FeSCN2+ (aq)
A big part of this lab includes understanding (and in the end proving) that absorbance is directly proportional to the concentration of a solution (Beer’s Law), and if Absorbance v. Concentration is graphed, a straight line will result. The regression line’s equation is used to determine the concentration of an unknown solution once the percent of T has been measured. The equation of Beer’s Law (A=abc) is an efficient way of …show more content…
Sources of uncertainty: Improper calibration of weighing balance, old chemicals used in the experiment.
CONCLUSION
In this lab, we determined equilibrium constant from the reaction between aqueous iron III nitrate and potassium thiocyanate, which was the purpose of the lab. Though the results were not exactly as expected, the data helped the students compute values that were close to the desired values. The results tended toward the uppers 100’s lower 200’s, which were near what was expected. Overall, the experiment was successfully performed and helped us to familiarize with the lab equipment, as well as learn how to deal with the contingency of the temperature value fluctuating due to environmental influences.
REFERENCES
[1] http://chemwiki.ucdavis.edu/Physical_Chemistry/Spectroscopy/Electronic_Spectroscopy/Electronic_Spectroscopy_Basics/The_Beer-Lambert_Law
[2] Beer.1852. Determination of the absorption of red light in colored liquids. Annalen der Physik und Chemie, vol. 86, pp.