After creating a Beer's Law plot using standard solutions of Q, you determined the slope of Beer's Law to be 0.543 M-1. Your unknown solution of Q tested in Part B of the experiment had an absorbance of 0.144. Determine the concentration (in molarity) of the unknown solution Q from Part B. Do not use scientific notation or units in your response. If Carmen adds zeros after the decimal place, your answer will still be graded correctly.

From the Beer's Law plot between absorbance and concentration we concldue that the slope is equal to [tex]\epsilon \times l[/tex] and path length is 1 cm.

As we are given that:

Slope = 0.543 M⁻¹

and,

Slope = [tex]\epsilon \times l[/tex]

[tex]\epsilon \times l=0.543M^{-1}[/tex]

[tex]\epsilon \times 1cm=0.543M^{-1}[/tex]

[tex]\epsilon=0.543M^{-1}cm^{-1}[/tex]

Now we have to determine the concentration (in molarity) of the unknown solution Q.

Using Beer-Lambert's law :

[tex]A=\epsilon \times C\times l[/tex]

[tex]0.144=0.543M^{-1}cm^{-1}\times C\times 1cm[/tex]

[tex]C=0.265M[/tex]

Therefore, the concentration (in molarity) of the unknown solution Q is, 0.265