Part 1- Calibration - the calculation of st of the Beer's Law Equation. In this part of the laboratory, you will calcula

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Part 1 Calibration The Calculation Of St Of The Beer S Law Equation In This Part Of The Laboratory You Will Calcula 1 (49.47 KiB) Viewed 35 times

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Part 1- Calibration - the calculation of st of the Beer's Law Equation. In this part of the laboratory, you will calculate the value of which is used in the Beer's Law equation (4) for determining the concentration, c, of FeSCN². In order to do this, we need to measure A and know the concentration, c, of FeSCN². We can get an excellent estimate of c by choosing initial concentrations which give nearly complete reaction in equation (1). Remember Le Chatlier's Principles. If the concentration of Fe³+ is increased, the equilibrium will shift to the right. A large excess of Fe³+ will cause a large shift in equilibrium to the right-essentially a "complete reaction". Note- You are calculating a single number to represent & .. Part 2- Determination of the Equilibrium Constant Value The reaction is repeated using lower concentrations of reactants to ensure that there is no very large excess of one reactant and that the reaction will now go to equilibrium. You can approach this much like you would a homework problem, using "x" to designate the equilibrium concentration of FeSCN2+. Thus, the absorbance from the colorimeter will allow us to calculate the concentration of the FeSCN²+ complex. We will use this, the 1:1 stoichiometry of the reaction, and the initial concentrations of the species to determine the equilibrium concentrations of the reactants and products and thus the equilibrium constant.
1) What is the concentration of iron (III) solution needed in Part 1? (Sig figs are important 2) What is the concentration of the iron (III) solution used later in Part 2?