Draw a calibration curve using the data set given below. Show and explain LOD and LOQ. Determine the dynamic linear range by examining the linearity of the absorbance measurements against Metal atoms concentration. Also Explain calibration methods. (hint: there are there types of methods. These are internal, external and standard addition methods) Metal, ppm Absorbance 0.220 0.044 0.440 0.090 1.100 0.228 2.200 0.465 4.400 0.932 6.600 1.187

.Express the following absorbances in terms of percent transmittance a) 0.0356 b) 0.379 0.167 c) 0.485

A solution in part C initially contains (4.2100x10^-4) molar SCN¯ and (3.1700x10^-3) molar Fe3+ This solution was then measured using the colorimeter, and an absorbance of (5.01x10^-1) was recorded.The constant determined in part A of the experiment was found to be (3.4800x10^3). Using the data provided above, determine the equilibrium concentration of Fe3+ [Fe3+ ]e in this solution. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer units

A student carries out the equilibrium constant experiment following a similar procedure used in the LearnSmart Lab simulator. In the first part of the experiment, there is a contaminant which causes absorbance values to read higher than they should for the thiocyanatoiron(III) complex. The resulting Beer's law plot has a slope that is larger than it would be if the contaminant was not present. This results in a Beer's Law plot with a slope that is larger than it would be if the contaminant were not present. If the same contaminant was not present when the student carries out the second part of the experiment, how will the student's results be affected? The molarities of thiocyanatoiron(III) ion would calculate higher and the calculated K. values would calculate higher. The molarities of thiocyanatoiron(III) ion would calculate lower and the calculated K. values would calculate lower. The molarities of thiocyanatoiron(III) ion would calculate higher and the calculated K. values would…

A student calibrated the mini-spectrophotometer with a blank solution, and then went to check their solution. They got a fingerprint on the cuvette while filling it. Because of this, the expected reading for the absorbance would be too high which would cause the calculated value of K, to be too high

A solution in part C initially contains (4.0300x10^-4) molar SCN¯ and (2.880x10^-3) molar Fe3+. This solution was then measured using the colorimeter, and an absorbance of (4.8600x10^-1) was recorded.The constant determined in part A of the experiment was found to be (3.40x10^3). Using the data provided above, determine the equilibrium constant for the reaction. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10 Answer

2. Do you observe any change in the form of the absorbance bands while moving from nonpolar to polar solvents?

Give answer all questions with explanation please

In an experiment you measure a solution absorbance of .2 with a path length of 1cm. If the molar absorptivity coefficient is 59cm-1 M-1 what is the concentration in molarity.

Please provide detailed explanation, thank you. I want to understand it.