Ve will only be doing calculations for Solution 1 going forward. You will o the calculations for Solutions 2 and 3 on your own. That should be elatively easier once we go through the calculation for Solution 1 here. Solution 1 calculations 1) Solution 1 contains 10.00mL of 0.002M iron (III) nitrate solution, 4.00mL of 0.002M potassium thiocyanate solution, and 6.00mL of 0.05M nitric acid solution. a) Calculate the concentration of iron (III) nitrate in the final solution in Solution 1. SHOW ALL WORK! b) Calculate the concentration of potassium thiocyanate in the final solution in Solution 1. SHOW ALL WORK! Amount of potassiom thiocyanate =900mL0.002H=0.000008mol concentrationofpotassiumthiocyanate=20.00mL0000008mol=0000004H Summarize the concentration of iron (III) nitrate and concentration of potassium thiocyanate in Solution 1 from your calculations in questions 1a and 1b above. You can fill in the same for Solutions 2-3 later after doing the calculations on your own time. You cannot do the limiting reagent thing here because you do not know that one reagent is in so much excess like before that the reaction will go to completion. So you must calculate the concentration of the [FeSCN 2] from the graph you created before. Is the absorbance value of Solution 1 within the range of values on the graph you created using the data from Phase 2 ? So can you use this absorbance value to determine the concentration of [FeSCN 2+ ] from the graph? (think about the definition of the slope and what the x and y axis are in this case and how it relates to the Beer-Lambert law). Doing the calculation to find the equilibrium constant Consider Solution 1 of Part 3. What is the concentration of iron (III) nitrate aka iron ( Fe3) ions in this tube? What is the concentration of potassium thiocyanate aka thiocyanate ions (SCN) ions in this tube? Refer back to the graph produced for the Pre-lab Assignment to solve for [FeSCN2+]