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?

Question

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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Answer 1

Explain Bot answered
7 months ago

To find the concentration of iron(II) in the unknown sample, we will use the equation for the calibration curve, which relates the absorbance (A) to the concentration of iron(II) ([Fe2+]). The equation given is:

A = 12.93 [Fe2+] + 0.0017

We are given the absorbance reading of the unknown sample, which is 0.106. We can substitute this value into the equation:

0.106 = 12.93 [Fe2+] + 0.0017

Now we can solve for [Fe2+] by rearranging the equation and isolating [Fe2+]:

12.93 [Fe2+] = 0.106 - 0.0017
[Fe2+] = (0.106 - 0.0017) / 12.93

Calculating this expression will give us the concentration of iron(II) in the unknown sample.

I hope this explanation helps!