5) Pd (II) forms a complex with acetylacetone (M M: 304.66g/mol Calculate the molar absorptivity of the complex given that a 82.50 ppm solution has a percent transmitte ince of 52.30% when measured in a 4.00 cm cell at a wavelength of 320 nm. A 259.69L/molcm B 482.50L/mol.cm C 1037.60L/mol.cm D) 3075.89L/molcm E) 761.07L/mol.cm

To calculate the molar absorptivity (ε) of the complex, we can use Beer-Lambert law, which states that the absorbance (A) of a solution is directly proportional to the concentration (c) of the absorbing species and the path length (l) of the light through the solution. The formula for Beer-Lambert law is:<br /><br />A = ε * c * l<br /><br />Given:<br />- Concentration (c) = 82.50 ppm = 82.50 mg/L<br />- Path length (l) = 4.00 cm<br />- Percent transmittance (T) = 52.30% = 0.5230<br /><br />First, we need to convert the concentration from ppm to moles per liter (M):<br /><br />c (in M) = (82.50 mg/L) / (Molar mass of Pd(acac)2) / 1000 mg/g<br /><br />c (in M) = (82.50) / (304.66 g/mol) / 1000 mg/g<br /><br />c (in M) = 0.0002706 mol/L<br /><br />Next, we can rearrange Beer-Lambert law to solve for molar absorptivity (ε):<br /><br />ε = A / (c * l)<br /><br />Since we have the percent transmittance, we need to convert it to absorbance (A) using the formula:<br /><br />A = -log10(T)<br /><br />A = -log10(0.5230)<br /><br />A = 0.284<br /><br />Now we can calculate the molar absorptivity:<br /><br />ε = 0.284 / (0.0002706 mol/L * 4.00 cm)<br /><br />ε = 261.19 L/mol·cm<br /><br />Therefore, the correct answer is:<br /><br />A) $259.69L/molcm$