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Lab 1: Equilibrium Constant Determination
You will have to determine the equilibrium constant for the reaction between aqueous iron(III) ion and thiocyanate ion. The equilibrium equation is given below:
Fe3+ (aq) + NCS– (aq) <---> FeNCS2+ (aq)
yellow colorless red
The absorbance of light is measured using a spectrophotometer. The higher the absorbance, the higher the concentration of FeNCS2+ present.
At room temperature, 5.00ml of 0.200M iron(III)nitrate solution was mixed with 5.00ml of 0.200M potassium thiocyante solution. The absorbance of this mixture was 0.55. A 1cm thick cuvette was used.
1- What is the Beer-Lambert Law?
The Beer-Lambert Law relates the attenuation of light to the properties of the material through which the light is travelling. In other words “The path length and concentration of a chemical are directly proportional to its absorption of light.” A = ԐCl
2. What is the path length (b) ? What is the molar extinction coefficient (E) ?
Slope= 5420.3
A =A0 + ԐCl
The slope is Ԑl.
Both the slopes will equal.
Ԑl = 5420.3
the cuvette is 1 cm in diameter that means the path length is also 1 cm. So,
Ԑl= 5420.3/1=5420.3 M−1cm−1
3. What is the equilibrium concentration of iron(III)thiocyante of our solution?
4. What are the equilibrium concentrations of Fe3+ and SCN- in our solution?
5. What is the equilibrium constant for the reaction at room temperature?
6. If we had used a temperature different the room temp, would that change our equilibrium constant? Explain your answer.
![Analysis of Fe-SCNequilibrium
y = 5420.3x - 0.0059
0.25
0.2
0.15
0.1
0.05
-0.05
0.0000
0.00002
0.000030.00004
0.00005
[Fe-SCN product] (M)
Abs @ 487 nm](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa0011cbe-4cc8-4b5d-a981-11b780b69bff%2Fefda066a-f2bc-43b5-b018-bdbc106edd87%2Fur4taeb_processed.jpeg&w=3840&q=75)
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