A student in 14CL performed theiron in vitamin experiment and obtained the follo

Question

A student in 14CL performed theiron in vitamin experiment and obtained the following Beer's Law set of data after complexation of the Fe in the multivitamin tablet with bipyridyl. weight of multivitamin tablet: 3.6632 g Absorbance Concentration (in g Fe/l) Solutions Standard 1 Standard 2 Standard 3 %T 72 0.142 0.178 0.212 0.321 5.4401 5.7283 6.0126 61 48 . Unknown iron solution The unknown iron solution was prepared by first dissolving the multivitamin tablet in hot HCI and then diluting the solution to the mark in a 50.00-ml volumetric flask with distilled water. The student then pipetted 10.00 mL of this solution into a 25.00-mL volumetric flask and also diluted it to the mark A 5.00-mL aliquot of the second solution was pipted into a 50.00-mL volumetric flask and 5.00mL of bipyridyl solution together with 5.00mL of buffer solution and 5mg of ascorbic acid were also transferred into the same 50.00-mL volumetric flask The resulting mixture in the 50.00-mL volumetric flask was finally diluted to the mark with distilled water The student went home and performed a linear regression analysis on this set of data. The equation of the line has the following form. Y= (0.1196 L g Fe) X (a) (8 points) Calculatete % Fe in the multivitamin tablet. Molecular weight of iron: 55.85g/mol.

Explanation / Answer

From above question , y= (0.1196)x , where this represents y=mx+c equation form and m=0.1196. Unknown concentration has absorbence of 0.321, applying A=ebc, 0.321= 0.1196 *1 * C C = 2.683 g/L   

% of Fe is 2.683/3.6632* 100 = 73.24%

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