You make a set of standards (solution of known concentration of the molecule/ions you want to determine), run them through the same procedure you will use on the unknowns, then measure the absorbance of each. Plot A on the y axis and mg/mL on the x axis. That is your calibration curve. Then you run the unknowns, measure A values, use the calibration curve to convert A to mg/mL and report your results.
I'm trying to do a lab, and I need to find the concentration of FeSCN+2 in five solutions based the calibration curve and the absorption. I have a calibration curve, the number of mLs and initial moles of Fe+3 and SCN-, the
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
Calibration data for a bromide ion-selective electrode (ISE) was collected and recorded below. The potential of the ISE was measured against a saturated calomel electrode (SCE). All solutions were buffered at a pH of 7.56. A
Calibration of a glass electrode gave a reading of 139.3 mV with 0.05 m potassium dihydrogen citrate buffer standard (pH = 3.766) and a reading of -79.0 mV with 0.08 m HEPES, 0.08 m NaHEPES, 0.08 m NaCl buffer standard (pH =
Melting point experiment: how do i know the calibration curve? we did an experiment where: week one we did a graph with the melting points of different compounds. week 2 we used the graph to correct the melting point of unknown #
Explain the following statement: "The validity of a chemical analysis ultimately depends on measuring the response of the analytical procedure to known standards." (b) Calibration curves are necessary in many chemical measurements