Introduction:
Haematinics are a group of medicines used to treat and prevent anemia, a condition characterized by a lack of healthy red blood cells or hemoglobin in the blood.
Hemoglobin is crucial for transporting oxygen throughout the body, and its deficiency can lead to symptoms like fatigue, weakness, shortness of breath, and dizziness.
Haematinics work by providing the essential nutrients required for the production of red blood cells and hemoglobin.
Key Components of Haematinics:
Iron: Vital for hemoglobin. Deficiency common in women and children. Supplements taken orally or IV.
Vitamin B12 (Cobalamin): Needed for red blood cell production and nervous system health. Deficiency leads to pernicious anemia, common in older adults and vegetarians.
Folic Acid (Vitamin B9): Essential for cell production, including red blood cells. Deficiency causes megaloblastic anemia, crucial for pregnant women to prevent birth defects.
Mechanism of Action:
Haematinics provide the necessary nutrients required for erythropoiesis, the process of red blood cell production in the bone marrow.
They help to:
Increase the availability of building blocks for hemoglobin synthesis.
Promote the proliferation and maturation of red blood cell precursors.
Correct nutritional deficiencies that may contribute to anemia.
Uses and Indications:
Iron Deficiency Anemia: Treatment and prevention, especially in high-risk groups.
Pernicious Anemia and Other B12 Deficiency States: Due to dietary deficiencies, absorption issues, or certain autoimmune conditions.
Folic Acid Deficiency: Prevention and treatment, particularly in pregnant women to prevent birth defects.
Some common types of anaemia include:
Iron-deficiency Anemia: Most common type, due to iron shortage for hemoglobin production. Causes include poor diet, bad absorption, or increased demand (e.g., pregnancy).
Vitamin-deficiency Anemia: Results from a lack of vitamins like B12 or folic acid needed for RBC production. Pernicious anemia is a B12 deficiency due to no intrinsic factor for absorption.
Haemolytic Anemia: RBCs are destroyed faster than made, due to inherited (e.g., sickle cell, thalassemia) or acquired reasons (e.g., autoimmune, infections).
Aplastic Anemia: Rare, severe type; bone marrow fails to make enough RBCs. Causes include radiation, certain drugs, or autoimmune diseases.
Chronic Disease Anemia: Linked to long-term illnesses (e.g., kidney disease, cancer) affecting RBC production/survival.
Haemorrhagic Anemia: From significant blood loss (trauma, surgery, heavy periods), depleting RBCs and iron.
Ferrous sulfate (FeSO4):
Preparation:
Ferrous sulfate can be prepared by reacting iron metal with dilute sulfuric acid, or by reacting ferrous oxide or ferrous hydroxide with sulfuric acid.
The chemical reactions are as follows:
Fe + H2SO4 → FeSO4 + H2 (using iron metal)
FeO + H2SO4 → FeSO4 + H2O (using ferrous oxide)
Fe(OH)2 + H2SO4 → FeSO4 + 2 H2O (using ferrous hydroxide)
Properties:
Ferrous sulphate is a greenish-white crystalline solid when hydrated (FeSO4·7H2O) and a white powder when anhydrous (FeSO4).
It is soluble in water and has a slightly acidic taste.
FeSO4 is an ionic compound and has a melting point of 70°C (158°F) for the heptahydrate form.
It is an oxidizing agent and can cause a reaction with reducing agents.
Uses:
Ferrous sulphate is used as a dietary supplement to treat iron-deficiency anaemia.
It is utilized in agriculture as a fertilizer to correct iron deficiencies in plants.
FeSO4 is used in water treatment for the removal of phosphates and as a coagulant.
It is employed in the manufacturing of inks, wood preservatives, and other chemicals.
Storage:
Ferrous sulphate should be stored in a cool, dry place, away from heat and direct sunlight.
It should be kept in a tightly closed container to minimize exposure to air and moisture.
Store FeSO4 away from strong oxidizing agents and reducing agents to prevent chemical reactions.
Assay
An assay of ferrous sulfate (FeSO4) typically involves a redox titration using potassium permanganate (KMnO4) as the titrant.
In short, the process can be summarized as follows:
Prepare a standard potassium permanganate (KMnO4) solution of known concentration.
Accurately weigh a sample of ferrous sulfate and dissolve it in distilled water, typically with the addition of a small amount of sulfuric acid (H2SO4) to maintain acidic conditions.
Heat the solution to about 60-70°C to ensure a faster reaction between the ferrous sulfate and potassium permanganate.
Slowly titrate the ferrous sulfate solution with the standardized potassium permanganate solution.
The ferrous sulfate will react with the potassium permanganate to form ferric sulfate (Fe2(SO4)3) and manganese(II) sulfate (MnSO4).
Continue adding potassium permanganate until a pale pink color persists in the solution, indicating the endpoint has been reached.
Calculate the concentration of ferrous sulfate in the sample using the volume of titrant used and the known concentration of the potassium permanganate solution.
Ferrous gluconate (C12H22FeO14):
Preparation:
Ferrous gluconate can be prepared by reacting ferrous sulphate with sodium gluconate. The chemical reaction is as follows:
FeSO4 + Na2C6H12O7 → FeC12H22O14 + Na2SO4
Properties:
Ferrous gluconate is a yellowish-gray to light green crystalline powder.
It is soluble in water and has a mildly sweet taste.
FeC12H22O14 is a non-toxic, biodegradable compound.
It has a melting point of about 180°C (356°F).
Uses:
Ferrous gluconate is used as a dietary supplement to treat iron-deficiency anemia.
It is often used in combination with other vitamins and minerals in multivitamin supplements.
Ferrous gluconate is also used as a food additive to fortify and enhance the iron content in various food products.
Storage:
Ferrous gluconate should be stored in a cool, dry place, away from heat and direct sunlight.
It should be kept in a tightly closed container to minimize exposure to air and moisture.
Store FeC12H22O14 away from strong oxidizing agents and reducing agents to prevent chemical reactions.