Pharmaceutical analysis- Conductometry

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    ✯Conductometry✯ 

• Conductometry is based on the principle of determination of change in conductivity.
• Change in the conductance is due to replacement of ions with each other.
• Ionic conductivity is different for different ions.

Conductance-; 

• Flow of electricity through electrolyte solution Due to migration a ions by applying potential differences between two electrode.

Electrode -; 

a. Anode ( positively charge , attract anions negative ions)
b. Cathode ( negatively charge attract, cation i.e. + ve ions)

It is indicated by G.

                       G= 1/R

Specific conductance-;

• It is reciprocal of specific resistance.

               R ∝ l/ a
              R= ρ×l/a  ( If l= 1m & a= 1m²)---- eq- 1
               R= ρ→ specific resistance

Equivalence conductance-;

• The conductance of 1gm equivalent solution is called equivalence conductance.

When , l = 1m , volume= 1m³ & 1gm equivalent solution is taken, then 
 
                   G= k = Aeq
                   Aeq = k× 1/ q   ( If 1gm equivalent solution)
                     Aeq = k

Molar conductance-;

• It is conductance of 1M solution.

                       λm = k× 1/ Cm     ( if m= 1)
                        λm = k

1. Conductivity meter-;

     It contains→ Digital display
                         → Calibrator
                         → power switch

2. Conductivity cell-;

• It is made up of by rex or quartz.
• It is fitted with two electrodes.
     1. Anode 
     2. Cathode
• Anode is +vely charge electrode it attract –ev ions.
• – ve ions are called anions.
• Cathode is – vely charge electrode it always attracts + ve ions.

3. Electrode-;

• Electrode are made up of platinum.
• Area & surface area of electrode are 1cm² & 1cm respectively.

Working-;

• Titrate the titrand i.e. ( CHჳCOOH) weak acid with titrant i.e. NH4OH by drop by drop with the help of burette.
• When titrant react with titrand salt formation takes place & ↑ the concentration of ions in solution.
• Ions are generated and conductivity is produced by ions , which is recorded by digital conductivity meter.

Conductometric  titration;

• Conductometric titration is a types of titration where electrolyte conductivity monitored continuously as one reactant is added .
• Equivalence point is the point at which the conductivity under goes sudden change.

Types-;

1 . Strong acid Vs strong base-;
• HCl used as strong acid.
• NaOH used as strong base
• HCl filled in Conductometric vessels.
• NaOH filled in burette.

      HCl  +  NaOH    →   NaCl   +.  HշO


2. Strong acid Vs weak base-;

• HCl as strong acid.
• NH4OH as weak base.
•  HCl in conductometry vessels & NH4 in burette.


     HCl   +   NH4OH    →     NH4Cl + HշO
          NH4Cl   →   NH4 ๋    +   Cl¯
       NH4OH      →        NH4 ๋    +    OH¯

3. Weak acid Vs strong base-;

• Weak acid is CHჳCOOH .
• Strong base is NaOH .
• CHჳCOOH in conductometry vessels and NaOH is burette.
 
 CHჳCOOH  + NaOH.   →.   CHჳCOONa. + HշO

4. Weak acid Vs weak base-;

• weak acid is CHჳCOOH .
•  weak base is NH4OH .
• CHჳCOOH filled in Conductometry vessels and NH4OH filled in burette.


CHჳCOOH + NH4OH  →   CHჳCOONH4 + HշO

           CHჳCOONH4  →   CHჳCOO¯ + NH4 ๋ 

         NH4OH      →       OH ¯ +  NH4 ๋


Application-;

• Use the check water pollution.
• Use in food microbiology for tracing micro- organism.
• Use to check alkalimetry of fresh water.
• Use to check salivity of sea water.
• tracing antibiotics.
• puring of distilled & di - ionised water.
• Basicity of organic acid.
• Solubility of sparingly soluble salts .


                       Thankyou

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