TO CARRY OUT THE CONDUCTOMETRIC TITRATION BETWEEN WEAK ACID (CH3COOH) AND STRONG BASE (NaOH)

APPARATUS REQUIRED:

• conductometer 

• Conductivity Cell

• Pipette 

• Measuring cylinder.

• Burette

• Beaker

CHEMICAL REQUIRED 

• CH3COOH Acetic acid 

• NaOH Sodium Hydroxide 

• Conductivity Water 

THEORY

Conductometric titration is one of the
electrometric methods of measurement of concentration of an electrolyte soln by finding out conductances at various stage of titration. It's curve is obtained by plotting graphically, the conductance against the volume of sol" added from the burette. The point of break of the point of intersection in the Conductometeric titration curve gives the end point of titration.

CH3COOH ➡️ CH3COO- + H+

CH3COO- + H+  + Na+  + OH- ➡️ CH3COO- +  Na+ 

 + H2O

Acetic acid is ionized feebly and the
conductance at zero addition of NAOH is low
on adding a small portion NAOH Solution. 

CH3COONA will be formed and the commanion effect of CH3COO- depress the lonization of acetic acid so conductance decreases but This initial depression is overcome by the high. concentration NAOH so that conductance increase slowly up to the equivalent point, and after equivalent point the addition of highly condudig 'Na+ and OH' makes the conductance to increase. Supply.The point of break in conductometric titration curve gives the equivalent point. 

In order to avoid the affect of dilution.
on conductance the concentration of the reagent soln of the burette should be at least 10 times greater than the concentration of the solutions of the Conductivity bottle.

PROCEDURE

clean burette was filled with O.1N NaOH solution pipette 10ml of the given acetic acid solution 100ml clean beaker and add about some of to make it approximately to time more dilute than the solution of the burrette. Conductivity cell was plated of known cell constant by dipping electrodes completely in the acid solution. Connected the cell to the conductivity bridge. Now we hour for record the conductance of diluted acid at every 0.5 ml addition of NaOH Soln with constant stirring Near to the equivalent point 0.2ml portions of NaOH are preferred. Conductometric titration is continued until the titration curve can be traced out clearly.

OBSERVATION

Concentration of NaOH(S) : 0.1N.
Volume of acetic acid pipetted (v₂): 50ml

Titration table

RESULT FROM CT. CURVE

The point of intersection of the curve the volume of NaOH solution of complete Nentalization(V1) = 5.5ml

CALCULATION

Name of S2 N acetic acid=V1 ml of 0.1N NaOH

Therefore, S2 = {V1×0.1÷V2} NaOH

                          = {5×0.1÷50} 

              i.e. S2 = 0.5÷50 

 Therefore S2 = 0.011N

RESULT

The concentration of acetic acid (weak acid) was found to be 0.011N

CONCLUSION.

Thus, we can carry out the conductometric titration between weak acid (CH3COOH) and strong base (NaOH).