Question

In this experiment, you will prepare a standard solution for a calibration curve for the formation of FeSCN2 complex by reaction different volumes of 0.002M Fe(NO,), and 0.002 M NaSCN. You will use 0.1M HNO, for all dilutions. Using the table, Calculate the equilibrium concentrations of FeSCN2+ Vol of Fe Vol of SCN 0.1 M HNO3 (mL) Equilibrium (mL) 10.00 10.00 concentration Fe[SCN] (mL) 0.00 1.00 2.00 3.00 4.00 5.00 10.00 9.00 8.00 7.00 10.00 10.00 10.00 6.00 5.00 10.00 Experiment 12 Le Chatelier's Principle: Chemical Equilibrium and Determination of Equilibrium Constant: Pre-Lab

Answer 1

To calculate the equilibrium concentrations of FeSCN2+, use the provided table and consider the changes in volume and initial concentrations of Fe and SCN-. Plug the values into the equation Fe³+ + SCN¯ → Fe(SCN)2+ to find the equilibrium concentration. For example, if the volume of Fe(NO3)3 is 0.00 mL and NaSCN is 5.00 mL, the equilibrium concentration of Fe(SCN)2+ would be 0.005 M.

Step-by-step explanation:

The equilibrium concentrations of FeSCN2+ can be calculated using the provided table. To determine the equilibrium concentrations, we need to consider the changes in volume and the initial concentrations of Fe and SCN-.

Let's take an example: for an equilibrium volume of 6.00 mL, the volume of Fe(NO3)3 is 0.00 mL and the volume of NaSCN is 5.00 mL. The initial concentration of Fe is 0.002 M, and the initial concentration of SCN- is also 0.002 M.

Using the equation Fe³+ + SCN¯ → Fe(SCN)2+, we can calculate the equilibrium concentration of Fe(SCN)2+ using the initial volumes and concentrations of Fe and SCN-. In this case, the equilibrium concentration of Fe(SCN)2+ would be 0.005 M.