Conductometric titration (Precipitation titration of KCl vs AgNO3 and BaCl2 vs Na2SO4)/Conductometry

Correction - In the second example BaCl2 vs Na2SO4.(Barium chloride and Sodium sulphate), (2-) charge should be given for the sulphate ion instead of (1-). in the equation

This video describes how to draw the conductometric titration curve for a strong acid with a strong base. It explains about the Conductometry, Principle of Conductometric titration. It explains how to draw the conductometric titration curve for the precipitation titration of KCl vs AgNO3 ( Potassium chloride and Silver nitrate) and BaCl2 vs Na2SO4.(Barium chloride and Sodium sulphate).
conductance is due to the movement of ions in the solution
one ion replaces with another ion of different ionic conductivity during the titration
equivalence point is determined graphically.
AgCl is a sparingly soluble salt- does not dissociate
Conductometric titration
(Analyte solution during titration
Before titration – only KCl present.
Presence of K+ and Cl- with low ionic conductivity – low conductance
During titration till equivalence point /neutralisation point–
AgCl (sparingly soluble salt) – does not dissociate
Cl- is replaced by NO3- with similar ionic conductivity – conductance remains constant.
At equivalence point/neutralisation point – AgCl and KNO3 are present
All KCl has reacted with AgNO3
After equivalence point – excess AgNO3 is added
accumulation of AgNO3 which can dissociate – conductance increases
equivalence point/neutralisation point is determined graphically
BaSO4 is a sparingly soluble salt -does not dissociate
Before titration – only BaCl2 present.
Presence of Ba2+ with high ionic conductivity – high conductance
During titration till equivalence point /neutralisation point–
Ba2+ with high ionic conductivity is replaced by Na+ with low ionic conductivity – conductance decreases
At equivalence point/neutralisation point – BaSO4 and NaCl are present
All BaCl2 has reacted with Na2SO4
After equivalence point – excess Na2SO4 is added
accumulation of Na+ and SO42- (can dissociate) in excess to Na+ and Cl- – conductance increases
Used for coloured solutions
Suitable for turbid solutions
Suitable for dilute solutions
System with incomplete reactions
Used for determining the concentration of weak bases and weak acids or mixture of acids
Special care is not required at the end point, as it is determined graphically
Does not require indicators.