2. In Part 1 of this experiment, you assumed that the FeSCN2+ concentrations in your

standard solutions were equal to the initial concentrations of SCN- ions. Now that you know the value of the equilibrium constant, calculate the actual equilibrium concentrations of Fe3+, SCN-, and FeSCN2+ in the mixture in test tube 2. Compare the values for the [FeSCN2+]. Are there any significant differences? Why or why not? (10 pts)

***HINT: Since you know the initial concentrations of your reactants, and you know Kc you can now solve for the equilibrium concentrations using an ICE table rather than a Limiting Reagent Table. Your Kc is large, not small; therefore, you cannot use the small x-approximation. You must solve the quadratic equation. Remember: One value of x will make more sense than the other.

Composition of solutions for praparing the calibration curve 1. Dbtain 15mL of 0.20Mfn(NO3)3 in 1MHNO5 and 2mL af 2.001023MKSCNaswellas12mL at Dl water. 2. There arn thron tast tubes (1-3) that nond to be labolad. 3. Pipette the indicated amounts of each solution into the test tube. 4. Mix asch salution thoroughly with a stir rod. 5. Make notes about what you observed. E. Use DI water to calibeate the spactrophotomater. 7. With each of the solutions shown above, use a dropper or pipette. B. Cach solution should be measured at 447nm for its absorbance. 9. Graph the data using the spreadsheet on canvas 10. On the datasheet, record the value of e including the correct units Part z: Composition of solutions for determining the equilibrium constant =6+4=0