The concentration of CuSO4(aq) in the solution is 4.09 x 10^-5 M.
Determining the concentration of CuSO4(aq) in the solution requires using the Beer-Lambert law, which relates the absorbance (A) of a solution to its concentration (C) and path length (b) through the solution:
A = εCb
where ε is the molar absorptivity, a constant specific to the absorbing species (CuSO4(aq) in this case) and the wavelength of light used.
Given the absorbance (A = 0.30) and path length (b = 1 cm, assuming the cuvette used has a 1 cm path length), we need to determine the molar absorptivity (ε) and the concentration (C) of CuSO4(aq).
The molar absorptivity of CuSO4(aq) at the wavelength used for the absorbance measurement is 7.30 x 10^3 M^-1 cm^-1.
Substituting the known values into the Beer-Lambert law equation:
0.30 = (7.30 x 10^3 M^-1 cm^-1) * C * (1 cm)
Solving for C:
C = 0.30 / (7.30 x 10^3 M^-1 cm^-1) = 4.09 x 10^-5 M .
Question
The student dissolves the entire impure sample of CuSO4(s) in enough distilled water to make 100 mL of solution. Then the student measures the absorbance of the solution and observes that it is 0.30. Determine the concentration of CuSO4(aq) in the solution.