D.PHARM (PART-I) SYLLABUS FOR PHARMACEUTICAL CHEMISTRY - I  
                                                                      (75 hours)  
                1)  General discussions on the following inorganic compounds  including     important 
                     physical  and  chemical  properties,  medicinal  and  pharmaceutical  uses  storage 
                     conditions and chemical incompatibility. 
                       a)  Acids,  bases  and  buffers  -  Boric  acid*,  hydrochloric  acid;  strong  ammonium 
                            hydroxide, calcium hydroxide, sodium hydroxide, and official buffers. 
                       b)  Antioxidants-Hypophosphorous  acid,  Sulphur  dioxide,  Sodium  bisulphite, 
                            Sodium meta bisulphite, Sodium thiosulphate, Nitrogen and Sodium Nitrite. 
                       c)  Gastrointestinal agents 
                            i)       Acidifying agents - Dilute hydrochloric acid 
                            ii)      Antacid  -  Sodium  bicarbonate,  aluminium  hydroxidegel,  aluminium 
                                     phosphate,  calcium  carbonate,  magnesium  carbonate,  magnesium 
                                     trisilicate, magnesium oxide, combinations of antacid preparations.  
                            iii)     Protectives and Adsorbent - Bismuth subcarbonate, Kaolin. 
                            iv)      Saline cathartics, Sodium Pottassium tartate and magnesium sulphate,  
                          d)  Topical agents 
                             i)      Protectives,  Zinc  Oxide,  calamine,  Zinc  stearate,  Titanium  dioxide, 
                                     Silicon polymers. 
                             ii)     Antimicrobials  and  Astringents-Hydrogen  peroxide*,  Potassium  . 
                                     permanganate. Chlorinated lime, iodine, Solutions of iodine, Providone-
                                     iodine,  Boric  acid,  Borax.  Silver  nitrate,  Mild  silver  protein,  Mercury, 
                                     yellow mercuricoxide, Ammoniated mercury. 
                             iii)    Sulphur  and  its  compounds  Sublimed  sulphur,  precipitated  sulphur, 
                                     Selenium sulphide. 
                             iv)     Astringents: Alum and Zinc Sulphate.  
              
                    e.  Dental  products  -  Sodium  fluroide,  stannous  fluoride,  Calcium  carbonate, 
                       sodiummetaphosphate, dicalcium phosphate, Strontium chloride, Zinc chloride. 
                    f.  Inhalants  - Oxygen, Carbon dioxide, Nitrous oxide. 
                    g.  Respiratory stimulants - Ammonium carbonate. Expectorants     and     Emetics - 
                       Ammonium chloride, Potassium iodide. Antimony Potassium tartrate. 
                       1)  Antidotes - Sodium nitrite 
                       2)  Major Intra and Extracellular eletrolytes.  
                             a)     Electrolytes  used  for  replacement  therapy-Sodium  chloride  and  its 
                                    preparations, Potassium chloride and its preparations. 
                             b)     Physiological acid base balance and electrolytes used, sodium acetate, 
                                    potassium  acetate,  sodium  bicarbonate  injection,  sodium  citrate, 
                                    potassium citrate, sodium lactate injection Ammonium chloride and 
                                    its injection 
                             c)     Combination of oral electrolyte powders and solutions. 
             3)  Inorganic  Official  compounds  of  Iron  Iodine,  and  Calcium  Ferrous  Sulfate  and 
                  calcium gluconate. 
             4)  Radio pharmaceuticals and Contrast media - Radio activity - Alpha, Beta and Gamma 
                  Radiations,  Biological  effects  of  radiations,  Measurement  of  radio  activity  G.M. 
                  Counter - Radio Isotopes - their uses storage and precautions with special reference to 
                  the official preparations. Radio opaque Contrast media-Barium sulphate. 
             5)  Quality  control  of  Drugs  and  Pharmaceuticals  importance  of  quality  control, 
                  Significant  errors,  methods  used  for  quality  control,  sources  of  impurities  in 
                  Pharmaceuticals, Limit tests for Arsenic, chloride, sulfate, Iron and Heavy metals. 
             6)  Identification tests for cations and anions  as per Indian Pharmacopoeia.  
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                                                          ACIDS, BASES AND BUFFERS 
                 Theories of Acid and Base 
                 Three important theories are 
                      1.  Arrhenius theory  
                      2.  Lowry and Bronsted theory 
                      3.  Lewis theory   
                 1.  Arrhenius Theory (Dissociation concept) According to this theory  
                                                                                                                    +
                         i.     Acid is a substance, dissociates to give hydrogen ions (H ) in water.  
                                                          H2O        +        - 
                                     eg:  HCl         ⎯⎯⎯→ H  + Cl
                                                                                                                     -
                         ii.    Base is substance, dissociates to give hydroxide ions (OH ) in water.  
                                                          H2O          +         - 
                                     eg:  NaOH ⎯⎯⎯→ Na  + OH
                 2. Lowry-Bronsted Theory (Proton Concept) 
                           According to them  
                         i.     Acids are called as proton donors which donates protons in solution to any other 
                                substance  
                         ii.    Bases are called as proton acceptors which accept protons in solution from any 
                                other substance.  
                                                                   +    - 
                                     NH +HCl  → NH Cl
                                           3                     4
                           In  the  above  reaction,  HCl  donates  a  proton  and  ammonia  accepts  that  proton 
                 forming ammonium chloride.    
                           So, according to this theory HCl is an acid and ammonia is a base. 
                 3. Lewis Theory (Electron Concept) 
                           Based on this theory, acids are called as electron acceptors which accept a lone pair 
                 of electrons. Bases are called as electron donors which donate a lone pair of electrons in 
                 solution.  
                           +                      + 
                 Eg : H  + NH  → NH
                                     3           4
                                                                               +
                           In  the  above  reaction,  proton  (H )  accepts  one  electron  pair  from  NH3  and  is 
                 therefore an acid, where as NH  molecule donates an electron pair is a base. 
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                                                                         BORIC ACID 
                                         M.F. H3 BO3  
                                         Syn : Ortho Boric Acid 
                 Preparation :  
                 (i) Laboratory Method  
                                                                                   3 
               
                       Adding a mixture of concentrated sulphuric acid and water to a boiling solution of 
              borax, the solution is allowed to cool. The boric acid is filtered and then washed until they 
              become free from sulphate ions.  
              Na  B O  + H SO  + 5H O → Na  SO  + 4H  BO   
                  2  4   7     2    4       2          2     4       3     3
              (ii) Commercial Method or Industrial Method 
                       It  is  prepared  commercially  by  decomposing certain naturally occurring borates 
              such as colemanite, resonite, borax, etc. eg. Cole manite is suspended in boiling water then 
              sulphur-di-oxide gas is passed through the suspension to liberate boric acid. 
              Ca  B  O . 5 H O  +  2SO  + 4H O 
                 2   6   11      2             2       2
              (Colemanite)   
                               6H BO   + 2 CaSO
                                   3    3              3  
                                             (Calcium Sulphite) 
              Physical Properties  
                  i.       White odourless, crystalline powder, soft to touch. 
                  ii.      Slightly acidic to taste. 
                  iii.     Freely soluble in boiling water, boiling alcohol and glycerin.  
              Chemical Properties  
                  i.       Boric acid is a weak acid. On heating to 100C loses one molecule of water to 
                           give meta boric acid. 
                                                 100C
                                  HBO  ⎯⎯⎯→ HBO + HO 
                                     3    3                        2     2
                                                       (metaboric acid)            
                  ii.      Upon further heating to 160C, further loss of water from metaboric acid to tetra 
                           boric acid. 
                                                160C
                                  4HBO  ⎯⎯⎯→ H BO + HO   (Tetraboric acid) 
                                          2                 2   4  7      2
                  iii.     On heating tetra boric acid produces the boric acid anhydride, boron trioxide 
                           BO 
                             2  3
                                                    160C
                                  H BO  ⎯⎯⎯→ 2BO    +  HO  
                                     2  4   7                    2  3            2
                                                          (Boron trioxide)            
                  iv.      One molecule of acid reacts with only one mole of sodium hydroxide. 
                               NaOH + H BO  → NaBO  + 2H O 
                                            3     3            2       2
              Assay  
                       Boric acid is assayed by titrimetric method. It is a very weak acid, hence it cannot 
              be titrated directly with a base to a sharp end point. It is dissolved in a mixture of water 
              and glycerin  and  it  is  made  as  strong  acid  i.e.,  Glyceroboric  acid  and  then  it  can  be 
              titratred  with  sodium  hydroxide  to  phenolphthalein  as  indicator.  The  end  point  is 
              appearance of permanent pale pink colour. 
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