The absorbance of a 6.3x10^-5M solution of an iron complex was measured to be 0.328 at the optimum wavelength. A second solution of the iron complex has an absorbance of 0.833 measured under identical conditions. What is the molarity of the complex in the SECOND SOLUTION?

Absorbance = kC

Plug in A and C from the first run and calculate k.
Use k and absorbance of second run to calculate C for second sample.

To determine the molarity of the complex in the second solution, you can use the Beer-Lambert Law. The Beer-Lambert Law states that the absorbance of a solution is directly proportional to the concentration of the absorbing species.

The equation for the Beer-Lambert Law is:

A = εcl

where:
A is the absorbance,
ε is the molar absorptivity (a constant unique to each substance),
c is the concentration of the substance in moles per liter (Molarity),
and l is the path length of the light through the solution (typically in centimeters).

In this case, you have the absorbance for the second solution (A = 0.833) and the molar absorptivity ε is assumed to be the same for both solutions since they contain the same iron complex. You do not have the path length, but it is stated that the conditions are identical.

To find the molarity (c) of the complex in the second solution, you rearrange the Beer-Lambert Law equation:

c = A / (ε * l)

Since the path length (l) is the same for both solutions, you can assume it cancels out and can be ignored. Therefore, you can calculate the molarity (c) as:

c = A / ε

Now you need the molar absorptivity (ε) of the iron complex. This value can be found in a reference source, such as a scientific literature or a database, specific to the iron complex you are studying.

Once you have the molar absorptivity (ε), you can substitute the values into the equation to calculate the molarity (c) of the complex in the second solution.