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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?

Part 1: Determination of an equilibrium constant at room temperature
The reaction in consideration is an equilibrium reaction
Fe3+(aq). + SCN&quot;(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&quot; 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 = &amp;. b. c. Where, &amp; = 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 = &amp; . C
The value of &quot;&amp;&quot; 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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