Class: Diploma in Pharmacy Subject: Pharmaceutical Chemistry 1st Topic: Official Compounds of Iron Includes the Importance of Iron, Iron Deficiency Anemia, Iron Poisoning and its treatment, Incompatibilities of Iron Compounds

1. P R E P A R E D B Y
MR. KAMBLE S. V.
M . P H A R M ( P H A R M A C E U T I C A L C H E M I S T R Y )
Official Compounds of
Iron

2. Content
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1. Importance of Iron in the body
2. Iron deficiency Anemia
3. Iron poisoning
4. Important iron compounds and preparations
5. Incompatibilities and Storage of Iron salts

3. Importance of Iron in the body
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 Iron is one of the essential constituent of the
body. The usual content is about 45 mg/kg of
body weight.
 In medicine iron is used in the form of its
compounds as Ferric salts (Fe+++) and Ferrous
salts (Fe++) and Complexed form.
 Sources: Vegetables, Milk, Whole grains.

4. 4
 The content of iron in the body is controlled by
regulating the absorption and not by excretion, as
the body recycles the iron obtained from the
breakdown of R. B. C. and thus the daily requirement
of Iron is quite low.
 Males (10-12 mg) & Females (12-18 mg)
 A small amount of iron is excreted into urine and
feaces (about 1 mg daily).
 The deficiency of Iron causes Iron deficiency anemia
 The elevated level cause Iron poisoning.
Importance of Iron in the body

5. Importance of Iron in the body
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 Iron is an essential constituent of blood system
and tissues where it plays a very specific role.
 It is usually associated with three types of
proteins:
i. Hemoproteins
Hemoglobin, Myoglobin, Cytochromes and other enzymes
Catalase and peroxidase
ii. Iron storage Proteins
Ferritin and Hemosiderin
iii. Transport Proteins
Transferrin

6. Hemoproteins
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 Hemoproteins are responsible for respiration and
for carrying oxygen.
 Hemoglobin, Myoglobin, Cytochromes and other enzymes
Catalase and peroxidase.
 In hemoglobin, iron is present in ferrous form
(Fe++) and it complexes with molecular oxygen.
 The uptake or release of oxygen depends on various
factors like pH, Carbondioxide etc.

7. Iron Storage Proteins
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 Ferritin and Hemosiderin are the important iron
storage proteins.
 These are found in liver, spleen and bone marrow.
 In Ferritin the complexed iron is present as a ferric
(Fe+++) form, but it is released in ferrous (Fe++) form.
 Hemosiderin is considered as dehydrates form of
Ferritin.
 The solubility of these two proteins is differ, ferritin
is water soluble and hemosiderin is water insoluble.

8. Transport Proteins
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 Transferrin, a glycoprotein present in blood plasma
as the major iron transport protein.
 Two atoms of ferric (Fe+++) ions are bound to each
molecule of glycoprotein so there is no free iron is
present in the plasma.
 The glycoprotein releases the iron to precursor of red
cell for the production of R. B. C.

9. Iron deficiency Anemia
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 The condition in which the capacity of the blood to
transport oxygen to tissues is reduced due to the
deficiency of Iron.
 Causes:
 Large amount of iron is lost in haemorrhage and in menstrual
flow.
 Iron requirement increases during pregnancy, growth and
lactation as it is transported to placenta.
 Due to inadequate absorption.

10. Iron deficiency Anemia
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 Treatment:
 Iron preparations along with cyanocobalmine.
 Large no. of oral preparations like liquids, capsules, tablets or
injectables are available in market.
 Injectables are rarely used as oral therapy gives satisfactory
results.
 The oral preparations sometimes cause constipation, GIT
irritation leads to vomiting and diarrhea.
 The side effects can be controlled by time of administration
and dose.

11. Marketed Iron Preparations

12. Iron Poisoning
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 The overdoses of iron preparations can cause serious
problems leading to death particularly young
patients.
 It is important to Keep iron preparations away from
children.
 Treatment:
 Usually treated by gastric lavage, followed by giving Sodium
bicarbonate and sodium dihydrogen phosphate which converts
iron into insoluble iron salts.
 If there is no evidence of kidney damage then deferoxamine is
orally administered to prevent the absorption of iron.

13. What is Lavage?
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14. Gastric Lavage
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15. Important Iron Comp. & Preparations
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1. Ferric Ammonium Citrate
2. Ferrous Fumarate
3. Ferrous Gluconate
4. Ferrous Succinate
5. Ferrous Sulphate and its preparations
6. Iron & Dextran Injection
7. Iron Sorbitaol injection

16. Action and Uses of Iron Preparations
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 The iron preparations are generally used as hematinic
(Substance that increases hemoglobin content).
 The choice of iron salts & preparations and dose depends
upon the extent of iron deficiency anemia.
 Ferrous sulphate is most commonly used iron prep. In the
form of tablets, coated or mixed with glucose or lactose to
prevent its oxidation.
 Ferrous sulphate mixture is also used for pediatric purpose.
 Ferrous Gluconate and ferrous succinate are used in the
form of tablets or capsules.

17. Action and Uses of Iron Preparations
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 Some of Iron preparations are used parenterally, e. g.
 Iron and dextran injection.
 Iron sorbitol injection
 They are alternative to oral preparations and increases iron
storage rapidly than oral preparations.
 They are used in diseases like Sprue in which iron
absorption from GIT is prevented and inflammation of
bowel occurs.

18. Doses of Iron Preparations
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 Ferrous fumarate 100 mg contains 32.5 mg iron and
usual dose is 200 – 600 mg daily.
 Ferrous gluconate 100 mg contains about 11.6 mg
iron and usual dose is 600 mg daily.
 Ferrous sulphate heptahydrate 100 mg, contains 20
mg iron and usual dose is 200 – 300 mg daily.
 Ferrous succinate 100 mg contains 35 mg of iron and
usual dose is 100 mg daily

19. Incompatibilities & Storage
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 Most of iron compounds & preparations are oxidized by air
and thus are stored in air-tight containers, in cool and dark
place.
 Ferric Ammonium Citrate:
It is incompatible with mineral acids, alkali, alkali carbonates and
tannates.
 Ferrous Gluconate:
It is stable in solutions buffered with citrate buffer to pH 3.5 – 4.5.
In alkaline and neutral solution it oxidizes.
The solution is incompatible with ascorbic acid, glycin & develops
dark color and with pyridoxine it becomes greenish.
 Ferrous Sulphate:
It is incompatible with alkali, phosphates, tannates, benzoates and
gets oxidized in air easily.

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