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OCR A-Level Chemistry PAG 12.1- Determining The Amount of Iron in Iron Tablets £5.49
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OCR A-Level Chemistry PAG 12.1- Determining The Amount of Iron in Iron Tablets

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  • February 10, 2021
  • 5
  • 2020/2021
  • Lecture notes
  • C
  • Pag 12.1

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12.1- Investigating the
Amount of Iron in an Iron tablet.

Introduction:
Iron tablets, medically known as ‘ferrous sulphate’, are
a supplement primarily containing around a standard
dosage of 200mg of the active ingredient iron (II)
sulphate (equal to 65mg of elemental iron), alongside;
maize starch, maltodextrin, calcium stearate, and red
dye (E124). The principal purpose for ferrous sulphate
supplements is to provide the necessary mineral that
forms red blood cells- iron2, to those who suffer a
deficiency. A scarcity of iron in the human body often
causes Anaemia, characterised by a plethora of
complications and symptoms- noticeable and subtle,
including but not limited to, constant lethargy and
fatigue, weakness, shortness of breath, headaches and
dizziness. To circumvent and avoid the aforementioned
symptoms and ailments, the necessary recommended
daily intake of iron stands at ~8.7mg for adult men,
and ~14.8mg for adult women3.
This investigation will determine the amount of iron
present in a standard tablet for treating Anaemia,
employing a redox titration methodology, wherein the
titrant-analyte pair react through means of oxidation-
reduction. In this case, the titrant-analyte are
potassium manganate (VII) and sulfuric acid,
respectively. The use of this titration will be in
determining the concentration of iron (II) ions in a
solution composed of crushed iron tablets, dissolved in
sulphuric acid. The redox reaction is expressed below.

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