In a conductometric titration, small volume of titrant of higher concentration is added stepwise to a larger volume of titrate of much lower concentration, and the conductance is measured after each addition.
The limiting ionic conductivity \(\left(\Lambda_0\right)\) values (in \(\mathrm{mS} \mathrm{m}^2 \mathrm{~mol}^{-1}\)) for different ions in aqueous solutions are given below:

For different combinations of titrates and titrants given in List-I, the graphs of 'conductance' versus 'volume of titrant' are given in List-II.
Match each entry in List-I with the appropriate entry in List-II and choose the correct option.

Option (P) :
On adding \(\mathrm{AgNO}_3\) solution to \(\mathrm{KCl}\) solution precipitation of \(\mathrm{AgCl}\) will occur due to which \(\mathrm{Cl}^{-}\)already present will be replaced by \(\mathrm{NO}_3^{-}\)ions. So conductance of solution will decrease till equivalence point. After complete precipitation of \(\mathrm{AgCl}\), further added \(\mathrm{AgNO}_3\) will increase the number of ions in resulting solution so conductance will increase.
Option \((\mathbf{Q})\) :
On adding \(\mathrm{KCl}\) solution to \(\mathrm{AgNO}_3\) solution precipitation of \(\mathrm{AgCl}\) will occur due to which already present \(\mathrm{Ag}^{+}\)ions will be replaced by \(\mathrm{K}^{+}\)ions in solution. So conductance of solution will increase. After complete precipitation of \(\mathrm{AgCl}\) further added \(\mathrm{KCl}\) will increase the number of ions in resulting solution so conductance will increase further.
Option (R) :
On adding \(\mathrm{HCl}\) solution to \(\mathrm{NaOH}\) solution, \(\mathrm{OH}^{-}\)will be replaced by \(\mathrm{Cl}^{-}\)ions so conductance of solution decreases. After complete neutralisation further added \(\mathrm{HCl}\) will increase number of ions in the solution. So conductance will increase further.
Option (S) :
On adding \(\mathrm{CH}_3 \mathrm{COOH}\) solution to \(\mathrm{NaOH}\) solution \(\mathrm{OH}^{-}\)will be replaced by \(\mathrm{CH}_3 \mathrm{COO}^{-}\)ions, so conductance of solution decreases. After complete neutralisation further added \(\mathrm{CH}_3 \mathrm{COOH}\) will remain undissociated because it is a weak acid and there is also common ion effect on acetate ions. So number of ions in solution will remain almost constant therefore conductance of solution will remain constant.