# How do we use the "Beer-Lambert law" to assess concentration?

$A = \epsilon b c$, where $A = \text{Absorbance}$, $\epsilon = \text{molar absorptivity}$, $b = \text{path length of cell}$, $c = \text{concentration of solution}$
And thus a plot of $A$ $\text{(y-axis)}$ versus $c$ $\text{(x-axis)}$ should yield a straight line. Your text will contain a whole section on this $\text{the Beer-Lambert Law}$, however, you will be able to see how good this law holds, by the straightness of your line, and how well the line of best fit intersects the experimental points.
Given the curve (which should be reasonaby linear), you can interpolate the PVA concentration from its measured $\text{absorbance}$ value. Does you agree?