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Determination of an Equilibrium Constant PART 1: Construction of a Calibration Graph Table 1: Absorbance of solutions with different volumes of SCN and HNO3 able[[Solutions, Absorbance],[1, 0.000],[2, 0.182],[3, 0.434],[4, 0.646],[5, 0.966]] PART 2: Determination of Keq for the formation of FeSCN2+ Table 2: Absorbance of solutions with different volumes of SCN and HNO3 able[[Solutions, Absorbance],[6, 0.000],[7, 0.138],[8, 0.278],[9, 0.423]] Molarity of Fe3+ solution in part 1 = 0.150M Molarity of Fe3+ solution (mL) = 0.00150M (in parts) Molarity of SCN in part 1 (mL) = 0.000500M Molarity of SCN in part 2 (mL) = (0.00300M) / 0.1 Molarity of HNO3 solution (mL) = 0.1M CALCULATIONS AND QUESTIONS Part 1: Construction of a Calibration Graph In a table, present the concentrations of FeSCN2+ (the complex) and absorbance values for solutions 1-5. Using Solution 2, show ONE sample calculation. Use Excel to construct a calibration curve (a plot of absorbance vs. concentration of complex), using solution 1 as a 0M standard. Perform a linear regression and display the equation for the best-fit line and the value of r^2 on the chart. Submit this graph with your lab report. Part 2: Determination of Keq for the Formation of FeSCN2+ Use the equation for the best-fit line and absorbance values to calculate the equilibrium concentration of the complex in solutions 7, 8, and 9 (show a sample calculation). Calculate the equilibrium concentration of Fe3+ and SCN- for solutions 7, 8, and 9 (show a sample calculation for Fe3+ concentration and a sample calculation for SCN- concentration). Calculate the equilibrium constant based on data for solutions 7, 8, and 9. From these, calculate the average value of the equilibrium constant for the formation of FeSCN2+.

          Determination of an Equilibrium Constant

PART 1: Construction of a Calibration Graph

Table 1: Absorbance of solutions with different volumes of SCN and HNO3
	able[[Solutions, Absorbance],[1, 0.000],[2, 0.182],[3, 0.434],[4, 0.646],[5, 0.966]]

PART 2: Determination of Keq for the formation of FeSCN2+

Table 2: Absorbance of solutions with different volumes of SCN and HNO3
	able[[Solutions, Absorbance],[6, 0.000],[7, 0.138],[8, 0.278],[9, 0.423]]

Molarity of Fe3+ solution in part 1 = 0.150M
Molarity of Fe3+ solution (mL) = 0.00150M (in parts)
Molarity of SCN in part 1 (mL) = 0.000500M
Molarity of SCN in part 2 (mL) = (0.00300M) / 0.1
Molarity of HNO3 solution (mL) = 0.1M

CALCULATIONS AND QUESTIONS

Part 1: Construction of a Calibration Graph

In a table, present the concentrations of FeSCN2+ (the complex) and absorbance values for solutions 1-5. Using Solution 2, show ONE sample calculation.

Use Excel to construct a calibration curve (a plot of absorbance vs. concentration of complex), using solution 1 as a 0M standard. Perform a linear regression and display the equation for the best-fit line and the value of r^2 on the chart. Submit this graph with your lab report.

Part 2: Determination of Keq for the Formation of FeSCN2+

Use the equation for the best-fit line and absorbance values to calculate the equilibrium concentration of the complex in solutions 7, 8, and 9 (show a sample calculation).

Calculate the equilibrium concentration of Fe3+ and SCN- for solutions 7, 8, and 9 (show a sample calculation for Fe3+ concentration and a sample calculation for SCN- concentration).

Calculate the equilibrium constant based on data for solutions 7, 8, and 9. From these, calculate the average value of the equilibrium constant for the formation of FeSCN2+.

determination of an equilibrium constant part 1 construction of a calibration graph table 1 absorbance of solutions with different volumes of scn and hno3 tablesolutions absorbance1 00002 01 33764

Added by Kelsey P.

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