In: Chemistry
Before working this pre-lab exercise read the theory, experimental precedures and sample calculations outlined in the laboratory manual. Suppose that a student collects the following spectrophotometric data to determine the relative concentrations of HMR and MR in solution: The abosorbance at 425 nm was measured to be 0.310 and at 520 nm was 0.770, the slopes corresponding to standard Beer's Law plots were as follows: αIA = 0.072 αIB = 0.306 αIIA = 0.760 αIIB = 0.036 Using this data, calculate the ratio between the relative concentrations of MR- and HMR in this solution.
The absorbance of the mixture of HMR and MR- at 425 nm = 0.310
at 520 nm = 0.770
According to beer law A = k c where k = beer law constant which is given by the slope of the beer law plot.
We know that the total absorbance in a mixture A = A1 + A2
where A1 = absorption due to component HMR
A2 = absorption due to component MR-
A1 = k1c1 k1 = beer law constant of component HMR A2 = k2c2 , k2 = beer law constant of component MR-
c1 = concentration of componet HMR c2 = concentration of component MR-
At wavelength 425 nm
A = 0.310 , k1 and k2 are 0.072 and 0.306 respectively
A1 = k1c1 = 0.072 c1
A2 = k2c2 = 0.306 c2
therefore 0.310 = 0.072 c1 + 0.306 c2 (or) 0.072 c1 + 0.306 c2 = 0.310 ----------------- (1)
similarly at wavelength 525 nm
A = 0.770 , k1 and k2 are 0.760 and 0.036 respectively
A1 = k1c1 = 0.760 c1
A2 = k2c2 = 0.036 c2
therefore 0.770 = 0.760 c1 + 0.036 c2 (or) 0.760 c1 + 0.036 c2 = 0.770 -------------------- (2)
solving (1) and (2)
0.072 c1 + 0.306 c2 - 0.310 = 0 ----------------- (1)
0.760 c1 + 0.036 c2 - 0.770 = 0 ----------------- (2)
c1 / [ -0.306 * 0.770 + 0.310*0.036] = c2 / [-0.310*0.760 + 0.072*0.770] = 1 / [0.072 * 0.036 - 0.306 * 0.760]
c1 / [ -0.23562 + 0.01116] = c2 / [ - 0.2356 + 0.05544] = 1 / [ 0.002592 - 0.23256]
c1 / -0.22446 = c2 / -0.18016 = 1 / -0.23
[MR- ] / [ HMR] = c2 / c1 = 0.18016 / 0.22446
= 0.80
Thus the ratio of relative concentrations of MR- and HMR in solution is 0.80