Question
The standard solution of FeSCN2+ (prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN) has an absorbance of 0.520.
If a trial's absorbance is measured to be 0.275 and its initial concentration of SCN– was 0.00060 M, what is the equilibrium concentration of SCN–?
If a trial's absorbance is measured to be 0.275 and its initial concentration of SCN– was 0.00060 M, what is the equilibrium concentration of SCN–?
Answers
Use the standard solution to calculate the constant a in Beer's Law of A = abc. You know A, b(the cell length) and c the concn.
Then the same A= abc to calculate concn from the unknown. You have A, you have calculated a from above, you have b and can calculate c, the concn of the unknown. You know how much SCN^ you started with the difference should be how muuch is left. you started with so
Then the same A= abc to calculate concn from the unknown. You have A, you have calculated a from above, you have b and can calculate c, the concn of the unknown. You know how much SCN^ you started with the difference should be how muuch is left. you started with so