pharmaceutical chemistry drug synthesis Pharmaceutical chemistry is the study of drugs, and it involves drug development. This includes drug discovery, delivery, absorption, metabolism, and more. There are elements of biomedical analysis, pharmacology, pharmacokinetics, and pharmacodynamics. Pharmaceutical chemistry work is usually done in a lab setting. what Does A Pharmaceutical Chemist Do? Pharmaceutical chemists are basically chemists in the pharmaceutical industry. They conduct research on drugs, formulate new drugs, and monitor the quality control of the drug making process.

2. Aluminium hydroxide:
Aluminum hydroxide is found in nature as the mineral Gibbsite
(also called hydrargillite) or Bayerite or Nordstrandite or Doyleite.
A mixed aluminum oxide-hydroxide mineral is known as diaspore or
boehmite.
In a purified form, aluminum hydroxide is either a white bulky
powder or granules with a density of about 2.42 g/mL. It is insoluble
in water, but soluble in strong acids and bases. Aluminum hydroxide
behaves as an amphoteric substance. That is, it acts as an acid in the
presence of a strong base and as a base in the presence of a strong
acid.

3. Properties:
PHYSICAL STATE Amorphous odorless white powder
MELTING POINT 300 C
SPECIFIC GRAVITY 2.42
SOLUBILITY IN WATER insoluble
SOLUBILITY IN ACID or BASE soluble
pH weak basic
STABILITY Stable under ordinary conditions

4.  Aluminum hydroxide is popular as an antacid. It behaves
as a base, reacting with and neutralizing excess stomach
acid (hydrochloric acid) to bring relief from "heartburn."
 Aluminum hydroxide is also used as a mordant in dyeing.
 Additional uses of aluminum hydroxide include the
manufacture of aluminosilicate glass, a high melting point
glass used in cooking utensils, the waterproofing of fabrics,
and the production of fire clay, paper and printing inks.
 Used as a raw material for fertilizers, and fibre cement
board products.
 As a flame retardant and smoke suppressant filler.
Uses:

5. Preparation:
Bauxite + 2NaOH → 2NaAlO2+H2O
175Oc - 270Oc
Virtually all the aluminium hydroxide used commercially is
manufactured by the Bayer process which involves dissolving
bauxite in sodium hydroxide at temperature 175-270°C. The
remaining solid, which is a red mud, is separated and
aluminium hydroxide is precipitated from the remaining
solution. This aluminium hydroxide can be converted to
alumina by calcinations.
2 H2O + NaAlO2 → Al(OH)3 + NaOH

6. Al2(SO4)3+6NaHCO3→ 3Na2SO4+2Al(OH)3+6CO2
Intermediate compound :
i) 2Al+3H2SO4→ Al2(SO4)3+3H2
ii) Solvay process
NaCl+CO2+NH3+H2O→NaHCO3+NH4CL

7. Magnesium hydroxide:
Magnesium is a naturally occurring mineral. Magnesium
is important for many systems in the body especially the
muscles and nerves. As a suspension in water, magnesium
hydroxide is often called milk of magnesia because of its
milk-like appearance. It also reduces stomach acid, and
increases water in the intestines which may induce
defecation.

8. Properties:
PHYSICAL STATE Crystalline, white powder, Odorless
MELTING POINT 350 C
DENSITY 2.3446 g/cm3
SOLUBILITY IN WATER Slightly soluble
SOLUBILITY IN DILUTE ACID soluble
pH
9.5-10.5
STABILITY Stable under ordinary conditions

9.  This is used for occasional constipation
 It is a laxative that is thought to work by drawing water into the
intestines, an effect that helps to cause movement of the
intestines.
 This medication is also used to treat symptoms caused by too
much stomach acid such as heartburn, upset stomach, or
indigestion. It is an antacid that works by lowering the amount
of acid in the stomach.
 Benefits of being on this drug can include regular bowel
movements, and relief from the painful symptoms of indigestion
 It is used as a filler in paper industry
 Its non-toxic character and high thermal stability make it an
attractive additive to polymers used to restrict polymers
flammability
 It is used as flame retardant composite
Uses:

10. Mg2+ (aq) + 2OH− (aq) → Mg(OH)2(s)
MgSO4(aq) + 2NaOH(aq) -------> Mg(OH)2(s) + Na2SO4 (aq)
Preparation:
Intermediate compound :
i) a) MgO(s) + H2SO4(aq) → MgSO4(aq) + H2O
b) MgCO3(s) + H2SO4(aq) → MgSO4(aq) + CO2(g) + H2O
ii) Ca(OH)2(aq) + Na2CO3(s) → CaCO3 → + 2 NaOH(aq)

11. Interactions
Magnesium hydroxide can decrease the absorption of drugs
such as:
•Tetracycline antibiotics (e.g., doxycycline, minocycline)
•Certain azole antifungals (e.g., ketokonazole, itraconazole)
•Quinolone antibiotics (e.g., ciprofloxacin, levofloxacin)

12. p-Aminosalicylic acid is a bacteriostatic agent remarkable
selective of pathogenic strains of tubercle bacilli causing
human tuberculosis.
History
In 1940 Bernheim first noticed that certain simple
chemical substances like benzoic acid and salicylic acid
would stimulate the consumption of oxygen of the
tubercle bacillus and increase its carbon dioxide
production, thus, changing its metabolism and affecting
its growth

13. Properties:
PHYSICAL STATE
Crystalline
odourless or has slight acetous odoer
White or nearly white powder
MELTING POINT 150-151 C
SOLUBILITY IN WATER soluble
pH of saturated aqueous solution 3.0-3.7
STABILITY In air blackish

14. PAS has nearly the same potency as streptomycin, but
considerably less potent. When it used alone, it shows
inferior beneficial effect to either streptomycin or
isoniazid. However, in combination with doses of
streptomycin or isoniazid, PAS enhances the clinical
response to full doses of these agents, or it permits
lower doses to be employed. Furthermore, and most
importantly, it delays the emergence of streptomycin
or isoniazid resistant strains of tuberculosis.
Uses:

16. Paracetamol also known as acetaminophen,
chemically named N-acetyl-p-aminophenol, is a widely
used analgesic (pain reliever) and antipyretic (fever
reducer). Acetaminophen is the name adopted for this
pharmacologic agent in the U.S. and Japan.
Paracetamol is classified as a mild analgesic. It is
commonly used for the relief of headaches and other
minor aches and pains and is a major ingredient in
numerous cold and flu remedies. In combination with
opioid analgesics, paracetamol can also be used in the
management of more severe pain such as post-surgical and
cancer pain.
Paracetamol

17. Properties:
PHYSICAL STATE
Crystalline powder
odourless and has bitter test
White powder
MELTING POINT 1690-1720 C
SOLUBILITY IN WATER
One part of paracetamol is soluble in 70
parts of water at room temperature, and
1 in 20 parts in boiling water
pH of saturated solution 5.5-6.5
STABILITY Stable in normal condition

18. Uses
• minor pain of arthritis
• backache
• the common cold
• muscular aches
• premenstural and menstrual cramps
• headache
• toothache
• temporarily reduces fever

19. Overdose or side effects:
This drug usually has no side effects. If you have any
unusual effects, contact your doctor or pharmacist
promptly.
 nausea, upper stomach pain, itching, loss of appetite
 dark urine, clay-colored stools; or
 jaundice (yellowing of the skin or eyes).

20. Synthesis:

21. Intermediate compound:
acetyl chloride sodium acetate acetic anhydride
Sodium borohydride

22. Ferrous sulphate
Ferrous sulfate is a salt with the formula FeSO4.
We normally get iron from the foods we eat. In
our body, iron becomes a part of our
hemoglobin and myoglobin. Hemoglobin
carries oxygen through our blood to tissues and
organs. Myoglobin helps our muscle cells store
oxygen. Ferrous Sulfate is an essential body
mineral. Ferrous sulfate is used to treat iron
deficiency anemia (a lack of red blood cells
caused by having too little iron in the body).

23. Properties:
PHYSICAL STATE
White crystals (anhydrous)
White-yellow crystals (monohydrate)
Blue-green crystals (heptahydrate)
Odourless
MELTING POINT
680 °C (anhydrous) decomposes
300 °C (monohydrate) decomposes
60–64 °C (heptahydrate) decomposes
SOLUBILITY IN WATER soluble
Specific gravity 1.898
STABILITY Oxidized by exposure to air

24.  Together with other iron compounds, ferrous sulfate is used to
fortify foods and to treat iron-deficiency anemia.
 Industrially, ferrous sulfate is mainly used as a precursor to other
iron compounds.
 It used as a reducing agent in cement factory.
 Ferrous sulfate was used in the manufacture of inks.
 It also finds use in wool dyeing as a mordant.
 In horticulture it is used for treating iron chlorosis.
 Ferrous sulfate is sometimes added to the cooling water flowing
through the brass tubes of turbine condensers to form a
corrosion-resistant protective coating.
 It is used in gold refining to precipitate metallic gold from auric
chloride solutions
Uses

25. The salt may be prepared by dissolving iron in diluted sulfuric acid.
The resulting solution is filtered and concentrated, if necessary, to
the point of crystallization of ferrous sulfate. Commercially, scrap
iron is used in the process.
In the finishing of steel plating or coating, the steel sheet or rod is
passed through pickling baths of sulfuric acid. This treatment
produces large quantities of iron(II) sulfate as a by-product.
Fe + H2SO4 → FeSO4 + H2
Another source of large amounts results from the production of
titanium dioxide from ilmenite via the sulfate process.
Ferrous sulfate is also prepared commercially by oxidation of pyrite:
2 FeS2 + 7 O2 + 2 H2O → 2 FeSO4 + 2 H2SO4
Synthesis:

26. Magnesium sulphate
Magnesium sulfate is a common pharmaceutical
preparation of magnesium, commonly known as
Epsom salt, used both externally and internally.
Epsom salt is used as bath salts and for isolation
tanks. Oral magnesium sulfate is commonly used as
a saline laxative or purgative. Magnesium sulfate is
the main preparation of intravenous magnesium.

27. Properties:
PHYSICAL STATE
colourless crystalline solid, odorless, bitter
taste
MELTING POINT
anhydrous decomposes at 1,124°C
heptahydrate decomposes at 150°C
SOLUBILITY IN WATER soluble (71 g/100 mL 20 °C)
STABILITY moisture sensitive

28.  Replacement therapy for hypomagnesemia
 Magnesium sulfate is the first-line antiarrhythmic agent for
cardiac arrest.
 Magnesium sulfate can be nebulized to reduce the symptoms of
acute asthma
 Solutions of sulfate salts such as Epsom salt may be given as first
aid for barium chloride poisoning.
 In gardening and other agriculture, magnesium sulfate is used to
correct a magnesium deficiency in soil; magnesium is an
essential element in the chlorophyll molecule.
 Anhydrous magnesium sulfate is commonly used as a desiccant
in organic synthesis due to its affinity for water
 Magnesium sulfate is used as the electrolyte to prepare copper
sulfate
Uses

29. Magnesium sulfate occurs naturally as the mineral epsomite,
MgSO4.7H2O. This is dissolved in water (usually hot) and the purified
sulfate is obtained by crystallization from solution. Industrially, the
crystals are centrifuged, dried and sieved.
It is also prepared from magnesium oxide. This is obtained by the
thermal decomposition of:
i) Magnesium hydroxide (obtained from sea water):
Mg(OH)2(s) → MgO(s) + H2O(g)
ii) Magnesium carbonate (from the ore magnesite):
MgCO3(s) → MgO(s) + CO2(g)
In either case, the oxide is reacted with sulfuric acid to produce
magnesium sulphate:
MgO(s) + H2SO4(aq) → MgSO4(aq)
Magnesium sulfate-7-water, MgSO4.7H2O, crystals are obtained by
evaporation. They may be recrystallised to increase purity.
Synthesis:

31. Brium sulphate
Barium sulfate is the inorganic compound with the
chemical formula BaSO4.
Properties:
PHYSICAL STATE white crystalline solid, odorless
MELTING POINT 1,580°C
SOLUBILITY IN WATER insoluble
STABILITY moisture sensitive

32.  Barium sulfate in suspension is frequently used medically
as a radio contrast agent for X-ray imaging and other
diagnostic procedures. It is most often used in imaging of
the GI tract
 The majority of synthetic barium sulfate is used as a
component of white pigment for paints
 A thin layer of barium sulfate called baryta is first coated
on the base surface of most photographic paper to increase
the reflectiveness of the image
 Barium sulfate is commonly used as a filler for plastics to
increase the density of the polymer
 Barium sulfate is used for testing pH in soil
Uses

33. Almost all of the barium consumed commercially is obtained from
barite, which is often highly impure. Barite is processed by carbo
thermal reduction (heating with coke) to give barium sulfide:
BaSO4 + 4 C → BaS + 4 CO In contrast to barium sulfate, barium
sulfide is soluble in water and readily converted to the oxide,
carbonate, and halides. To produce highly pure barium sulfate, the
sulfide or chloride is treated with sulfuric acid or sulfate salts:
BaS + H2SO4 → BaSO4 + H2S
Synthesis: