Beer-Lambert Law Practice Test

A student prepares a solution of a blue dye and measures its absorbance at 620 nm in a 1.00 cm cuvette. The molar absorptivity of the dye at this wavelength is $\varepsilon = 250\ \text{L mol}^{-1}\text{cm}^{-1}$. If the measured absorbance is $A = 0.500$, what is the concentration of the dye solution?

Two solutions of the same dye are measured at the same wavelength using identical 1.00 cm cuvettes. Solution 1 has concentration $1.0\times10^{-4}\ \text{M}$ and absorbance $A_1 = 0.30$. Solution 2 has concentration $3.0\times10^{-4}\ \text{M}$. Assuming Beer–Lambert law holds, what is the expected absorbance $A_2$ for Solution 2?