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1. Your boss advises you try to dissolve the tablet first in 100mL of DI water. Your sample is a complexmixture of dye, analyte, and filler material. Provide a reasonableargument using what you know aboutsolubility and chemistry, to convince a coworker or your boss thatall is not lost if the sample looks to not completelydissolve.2. Estimate the MDL of the Fe-bipyridyl method as three times thestandard deviation of a method blank, analyzed at 522 nm.Absorbance values of a method blank and the equation of thecalibration line are given in the table below. The correct answerto this question will serve as the estimated MDL needed to prepareyour MDL standard iron solution for the experiment. Hint: For thepurpose of maintaining correct significant figures, the calculationshould be done by converting A to concentration units beforecalculating for the MDL. The calibration equation was generated bymeasuring standard solutions (units: ppm) (x-values) and measuringtheir absorbance (y-values).Blank Aliquot Absorbance1 -0.0032 0.0033 0.0014 -0.0015 0.0016 0.0007 0.002Calibration Equation: y = 0.166812x - 0.006663. One pill of the iron supplement was crushed with mortar andpestle. The result was slurried with a few mL of DI water, and thenquantitatively transferred to a 100 mL volumetric flask. Beforediluting to the mark, a little HCl was added to ensure fulldissolution of the iron material. After mixing, 1.00 mL of thestock sample solution was diluted to 100 mL using a volumetricpipet and a 100 mL volumetric flask. If we use a 40.00 mL aliquotto prepare the sample, estimate the concentration of the resulting,100 mL solution. Will this concentration fall within our currentset of planned standards (see below)? Use math to justify youranswer.
4. Calculate what the estimated increase in iron concentrationshould be if a 1.00 mL spike of ~100 ppm Fe is used for the spikerecovery test. This question only addresses the general calculationfor the spike.
PLEASE ANSWER THIRD AND FOURTH QUESTION ONLY