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Part 1: Determination of an equilibrium constant at room temperature The reaction in consideration is an equilibrium reaction Fe3+(aq). +...
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  • How do you Calculate equilibrium concentration of FeSCN2+ complex?
  • The initial concentration of Fe3+ and SCN- can be calculated using dilution formula M1V1 = M2 V2 (Since the original concentrations of the solutions were given)
  • Using RICE table (or ICE table) how can you find the equilibrium concentration of Fe3+ and SCN-
  • In the end how can you find Kc for each dilution?

Screen Shot 2020-06-20 at 3.11.45 AM.png
Part 1: Determination of an equilibrium constant at room temperature
The reaction in consideration is an equilibrium reaction
Fe3+(aq). + SCN"(aq) = FeSCN2+(aq)
(colorless) (colorless)
(Blood Red)
For this experiment, a colorless 2.0 x10-3 M aqueous solution of Iron (III) nitrate (Fe(NO3)3) (colorless) was mixed with a 2.0 x10-3 M colorless solution of potassium thiocyanate (KSCN) which results in the formation of FeSCN2+ (blood red in color). Note the
reaction is in equilibrium. The purpose of this experiment is to find the equilibrium constant.
In this experiment, different combinations of Fest and SCN" were made as shown in the table. The solutions were allowed to settle for 5 min, assuming after 5 min the reaction has achieved equilibrium. At equilibrium, the absorbance of each solution was checked
using a micro lab instrument. The data was collected at 425 nm. With the absorbance value concentration of FeSCNZ complex can be determined (Beer's law).
A = &. b. c. Where, & = Molar absorptivity ; b = path length; c = concentration
Since path length is constant considering the same cuvette was used to check absorbance. Therefore, the above equation can be written as
A = & . C
The value of "&" is given in lab handout.
Use the following data
Sample ID
Total Volume (mL)
Abs @ 425 nm
Trial 1
4 mL Fe 3+ 5 mL SCN-
9
1.22
Trial 2
6 ml Fe3+ and 4 ml SCN-
10
1.18
Trial 3
8 mL Fe3+ and 2 ml SCN-
10
0.89

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