Can someone please answer 8,9,10 for me please I am so lost with these
together as the initial solution, what will be the initial concentration of SCN (aq)? 8. According to the equation Fe"(aq) + SCN(aq)ä¸[Fe(SCN)12"(ag), lf 1.0 mL of 0.002 M Fe3 (aq), 1.0 mL 0.002 M SCN-(aq) and 8.0 mL of H20 are mixed together as the initial solution, what will be the initial concentration of [Fe(SCN)]2+ (aq)? 9. In the calibration part of the experiment (Part 1), the reactants are combined with one as a limiting reagent. According to the equation Fe (aq) +SCN(aq)[Fe(SCN)12+(aq), if 1.0 m of 0.2 M Fe3 (aq), 1.0 mL 0.002 M SCN-(aq) and 69.0 mL of H20 are mixed together as the initial solution, what will be the equilibrium concentration of Fe3 (aq)? 10. In the calibration part of the experiment (Part 1), the reactants are combined with one as a limiting reagent. According to the equation Fe"(aq) + SCN(aq) = [Fe(SCN)]"(aa), if 1.0 mL of 0.2 M Fe3 (aq), 1.0 mL 0.002 M SCN (aq) and 69.0 mL of H2O are mixed together as the initial solution, what will be the equilibrium concentration of SCN(aq)? Safety Nitric acid, HNOs, is a strong acid. Wash all splashes and spills with copious quantities of water Procedure solutions Part 1: Calibration curve using standard Fe(SCN 1. Prepare solutions A-1 through A-6 using the instructions below. The instructor may divide t of chemicals used. Check with the instructor which solutions to make before you begin. Note that the concentration of the Fe solution used in this step is 0.100 M - make sure you class into groups, each group preparing 50 mL of one or two A solutions to minimize the am
3. You have been told that the reaction you are observing is:
Fe3+ (aq) + SCN-â (aq) â FeSCN2+ (aq)
Another possibility is that the reaction is:
Fe3+ (aq) + 2 SCN-â (aq) â Fe(SCN)2+ (aq)
Write the equilibrium equation for this new reaction.
Using your data from the mixtures in test tubes 1, 3, and 5 of Part 2, recalculate three new equilibrium constants for this new possible reaction. Hint: Notice that the change in concentration of SCN- in your equilibrium table will change because of the new stoichiometry. Also, the exponent on [SCN-] in the equilibrium constant expression will change for the same reason.
What are the three new equilibrium constants?
Why do the results of your calculations show that the reaction you are observing is more likely to be the first one (one mole of SCN- with one mole of Fe3+)?
4. In Part 1 of this experiment, you made the assumption 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 mixture in test tube 2. How good was the assumption? Did this satisfy the 5% rule (the loss of reactant is less than 5% of its initial concentration)?
