Question

A student based the analysis of Cu(II) in a sample on the formation of the blue complex [Cu(H2O)6]+2. A standard solution was made when 1.432 g of pure copper wire (MM= 63.546g/mol) was weighed, dissolved in concentrated HNO3, and diluted to 1.00x102 mL. The stock solution was used to make a dilution by mixing 6.00 mL of stock solution with 44.0 mL of deionized water. Colorimetric determination gave that the absorbance of the sample was 0.07525 when the path length of the light through the solution was exactly 1 cm. Calculate the transmittance of the solution.

Answer 1

The transmittance of the solution is 84,1%

Step-by-step explanation:

Uv-Vis absorbance is an important method to quantify different compunds as metals or some specific organic and inorganic compounds.

The absorbance relation with transmittance is:

A = 2 - log₁₀ %T

Where A is absorbance and %T is transmittance percent.

As the absorbance of the solution was 0,07525:

0,07525 = 2 - log₁₀ %T

-1,92475 = - log₁₀ %T

1,92475 = log₁₀ %T

84,1 = %T

Thus, the transmittance of the solution is 84,1%

I hope it helps!