Chemistry
posted by Ann .
Do I solve this by multiplying 1.8645 by 1.14??The equation of your calibration curve from a spectrophotometry experiment was y = 1.8645x. Assuming your calibration curve is set up exactly like it was in lab (concentration in mM on the x axis and absorbance on the y axis), what would the concentration of a solution be if the measured absorbance was 1.14A?

The equation of straight line is y = mx + b and this one is y = 1.8645x
y = absorbance; x = concn in mM = C.
Then 1.14 = 1.8645*C
Solve for C.
C = 1.14/1.8645 
The equation of your calibration curve from a spectrophotometry experiment was y = 1.8645x. Assuming your calibration curve is set up exactly like it was in lab (concentration in mM on the x axis and absorbance on the y axis), what would the concentration of a solution be if the measured absorbance was 0.92A?