ge 70 SOLUTION 5. The following data were obtained for a calibration (Beer\'s La
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ge 70 SOLUTION 5. The following data were obtained for a calibration (Beer's Law) plot. Molarity Absorbance 015 030 045 060 .075 037 .067 099 131 -167 2 Enter this data into Logger Pro (molarity will be X and absorbance will be Y). Perform a linear regression, L.e. determine the equation of the straight line that best fits the data (see Graphing exercise, page 24) Record the slope and intercept of the line of best fit: M (slope): = -4-1-le0alm b(intercept) Record the "goodness of fit" parameters: Corelation 6,99RMSE- In the equation y mx + b, y is the absorbance and x is the concentration (molarity). From the equation you have determined, calculate the concentration of a solution that has a measured absorbance of 0.111Explanation / Answer
According to the Beer's law,
Absorbance,A= LC, where C is concentration of solute and L constant for a particular experimental set up.If draw a plot of A vs C then it would be a straight line with slope m=L.
C then would be given by C=A/m.
Here A = 0.111 and m=2.16. Thus C=0.111/2.16= 0.0514M.
Thus concentration when absorbance is 0.111 is 0.0514M.
Comment in case of any doubt.
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