Refer to Table 2, test solution 3 in the procedure. At equilibrium, the concentration of the FeNCS2+ is determined to be 1.5 x 10-4 M in 10.0 mL total volume of solution. a. Calculate the number of moles of Fe3+ and SCN- added. b. Calculate the number of moles of FeSCN2+ formed. c. Calculate the number of moles of each reactant present at equilibrium. moles at equilibrium = initial moles - moles used up d. Calculate the concentrations of all species at equilibrium.  e. Calculate K.

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 Refer to Table 2, test solution 3 in the procedure. At equilibrium, the concentration of the FeNCS2+ is determined to be 1.5 x 10-4 M in 10.0 mL total volume of solution.
a. Calculate the number of moles of Fe3+ and SCN- added.
b. Calculate the number of moles of FeSCN2+ formed.
c. Calculate the number of moles of each reactant present at equilibrium. moles at equilibrium = initial moles - moles used up
d. Calculate the concentrations of all species at equilibrium. 
e. Calculate K.

B. Equilibrium Test Solutions
1. Prepare the test solutions according to Table 2 using small beakers.
Table 2
Test Solution
Vol. of 0.002 M
Vol. of 0.002 M
Vol. of 0.1 M
Absorbance at
Fe(NO3)3 (mL)
NaSCN (mL)
HNO3 (mL)
447 nm
1
1
4
3
3
3
2 T
4
4
1
2. Measure the absorbance of each solution at 447 nm.
5
2.
5
Transcribed Image Text:B. Equilibrium Test Solutions 1. Prepare the test solutions according to Table 2 using small beakers. Table 2 Test Solution Vol. of 0.002 M Vol. of 0.002 M Vol. of 0.1 M Absorbance at Fe(NO3)3 (mL) NaSCN (mL) HNO3 (mL) 447 nm 1 1 4 3 3 3 2 T 4 4 1 2. Measure the absorbance of each solution at 447 nm. 5 2. 5
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