The equation for a normal calibration curve for the detection of iron(II) is determined experimentally to be 𝐴 = 12.93 𝑀−1 [𝐹𝑒 2+] + 0.0017 Analysis of a sample with unknown concentration gives an absorbance reading of 0.106. What is the concentration of iron(II) in the unknown?
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8.06 mM
To determine the concentration of iron(II) in the unknown sample, we can use the equation for the calibration curve:
A = 12.93 [Fe2+] + 0.0017
We are given the absorbance value from the unknown sample, which is 0.106. We can substitute this value into the equation and solve for [Fe2+].
0.106 = 12.93 [Fe2+] + 0.0017
To isolate [Fe2+], we subtract 0.0017 from both sides of the equation:
0.106 - 0.0017 = 12.93 [Fe2+]
0.1043 = 12.93 [Fe2+]
Now, divide both sides of the equation by 12.93 to solve for [Fe2+]:
0.1043 / 12.93 = [Fe2+]
Using a calculator, we find:
[Fe2+] ≈ 0.00806 M
Therefore, the concentration of iron(II) in the unknown sample is approximately 0.00806 M.