Spectrophotometric Determination of Iron in Vitamin Tablets this is background i

Question

Spectrophotometric Determination of Iron in Vitamin Tablets

this is background information for the question? why did we add each of this compounds?

Place one tablet of the iron-containing vitamin in a 125-mL flask or 100-mL beaker and boil
gently (in a fume hood) with 25 mL of 6 M HCl for 15 min. why did we add HCL?

Fe standard into a 100-mL volumetric flask and add the same number of drops of citrate solution as required in step 2. Add 2.00 mL of hydroquinone solution and 3.00 mL of o-phenanthroline solution

what happens at each step and why did we add Fe standard then citrate solution then hydroquinone and finally o-phenanthroline solution Include the reaction equation for each or overall process.

Explanation / Answer

In this experiment, first of all HCl is added in the Fe containing vitamin tablet to digest the cellulosic matrix of the tablet in the process

As the experiment proceeds the Fe+3 is then reduced to Fe2+ with hydroquinone.(this will allow the reduction of iron)

While freshly-dissolved aqueous Fe2+ formed which is nearly colorless, it imparts an intense red color byundergoing a stoichiometric reaction of Fe2+ with three molecules of the ligand 1,10-phenanthroline (phen) forming the complex Fe(phen)32+.

Thus all these addition of the chemicals is used to detemine the mass of iron that was present in the vitamin tablet

Construction of a calibration curve using standard solutions allows to determine both the molar absorptivity of the Fe(phen)32+ complex and, with a pair of measurements of the iron tablet solution's absorbance under the same conditions, the mass of iron is also determined present in the vitamin tablet.

Reaction pdf is mailed to Ankit Saxena (Assistant- TMK | Chegg India Pvt. Ltd.)

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