Please answer question 1 and 2 thanks

Calculations: Before heading into the lab, please make sure you have done the following calculation. Calculate the mass of Fe(NH2)2(SO4)26H2O required to produce 500cm3 of a Fe (II) solution with a concentration of 0.04mg/cm3 or 0.04g/L. Note: concentration can be expressed in units of moldm3(M) or mg of sample per cm3 of solution, i.e., mg/cm3. Note, the numerical solution to this calculation is 0.141g, but you will have to show the procedure that allowed you to obtain this value. Experimental Consult a demonstrator as to the correct way to handle the cuvette cells and the operation of the spectrophotometer. When using solutions of o-phenanthroline, hydroquinone and sodium citrate, DO NOT pipette directly from the containers as this contaminates the solutions. Pour some into a small beaker first. Part A: Preparation of the Vitamin Tablets for Analysis. Place one of the iron-containing vitamin tablets in a 100cm3 beaker and add 25cm3 of 6.0moldm : 3HCl. Boil gently (in a fume hood) for about 15min. Before removing from the fume hood add 20 cm3 of cold deionised water to cool the solution. Filter the solution directly into a 100cm3 volumetric flask, rinsing the beaker several times with small portions of distilled water to ensure complete transfer of the iron. Allow the solution to cool, dilute to the mark and mix well. Label this solution "unknown 1".. As this solution is too concentrated in Fe(II), it must be diluted, otherwise the absorbance of the complex solution would be too high. It is good practice to keep the absorbance below 1.0, to ensure the validity of the Beer-Lambert Law, see Equation 3. To prepare the diluted sample, pipette 10cm3 of " unknown I' into a clean 100cm3 volumetric flask and dilute to the mark with distilled water. Label this solution " unknown 2 ". Pipette 10cm3 of " unknown 2 into 225cm3 beaker and find out how many drops of sodium citrate solution is required to bring its pH to approximately 3.5. Pipette another 10cm3 of the "unknown n into a clean 100cm3 volumetric flask, add the required amount of sodium citrate, 2cm3 of hydroquinone, 3.0cm3 of phenanthroline, dilute to the mark with distilled water and mix well. Label this solution " unknown 3 ". Allow the solution to stand for 10min and measure the absorbance at 508nm. Part B: Preparation of the Fe(II) standard solutions Accurately weigh out the correct amount of the Fe(NH4)2(SO4)26H2O salt to make 500cm3 of a 0.04 g/LFe (II) solution (see calculation above). Dissolve the salt by adding approximately 50cm3 of distilled water and 0.5cm3 of 98%H2SO4 (transfer the concentrated acid to the solution in the fume hood) and make up to 500cm3 in a volumetric flask. Label this solution "standard". Pipette 10cm3 of this " standard" into 25cm3 beaker and measure the pH of the solution with pH meter. Count the drops of sodium citrate required to bring the pH to approximately 3.5. Pipette a further 10cm3 of the "standard" into a clean 100cm3 volumetric flask and add the same number of drops of citrate solution. To this add 2.0cm3 of hydroquinone solution and 3.0cm3 of ophenanthroline solution and make up the mark with distilled water. Mix well and label this "standard 10 ". Repeat the procedure using 5.0cm3 and then 2.0cm3 and finally 1.0cm3 of the "standard'. In each case adjust the amount of citrate needed proportionately. Use 2.0cm3 of hydroquinone and 3.0 cm3 of o-phenanthroline for each one and dilute as before with distilled water. Label these solutions as " standard 5", "standard 2" and " standard 1 ". Prepare a blank solution (i.e., containing no Fe(II), containing 2.0cm3 of hydroquinone, 3.0cm3 of o-phenanthroline and dilute to the 100cm3 ) as before with water. Allow all solutions to stand for 10min and measure the absorbance at 508nm. Question 1. Calculate the mass of Fe(NH4)2(SO4)2.6H2O(392.13g/mol) required to produce 500cm3 of a Fe (II) solution with concentration 0.04mg/cm3. Convert this concentration to (i) ppm (ii) M Question 2. Calculate the concentration of iron (mg/cm3) in each of the "standard" solutions, which will be prepared during this experiment