Based on the calibration curve for the absorbance of nickel(II) sulfate on the l

Question

Based on the calibration curve for the absorbance of nickel(II) sulfate on the last slide of your handout, an unknown solution with an absorbance of 0.406 would have what molarity? (Do NOT write units)

Y=1.33x + 2E-16

r^2=1 Some answers will be used more than once. Directly related to the amount of light received by the detector. Inversely related to the concentration of a sample Directly related to concentration italic epsilon b c minus log open parentheses straight I over I subscript 0 close parentheses straight I over straight I subscript 0 x 100 The variable in Beer's Law that represents how an analyte responds to a given wavelenght. absorptivity path length A. b B. Absorbtion C. italic epsilon D. percent transmittance

Explanation / Answer

Equation from the calibration curve for the determination of Ni(II)SO4 is,

y = 1.33x + 2 x 10^-16

with,

y = absorbance

x = molar concentration of Ni(II)SO4

Now we have,

absorbance for the unknown (y) = 0.406

So,

molarity = (0.406 - 2 x 10^-16)/1.33 = 3.052

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