Question

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 ($\Lambda_{0}$) values (in $\mathrm{mS~m}^{2}\mathrm{~mol}^{-1}$) for different ions in aqueous solutions are given below:

| Ions | $\mathrm{Ag}^{+}$ | $\mathrm{K}^{+}$ | $\mathrm{Na}^{+}$ | $\mathrm{H}^{+}$ | $\mathrm{NO}_{3}^{-}$ | $\mathrm{Cl}^{-}$ | $\mathrm{SO}_{4}^{2-}$ | $\mathrm{OH}^{-}$ | $\mathrm{CH}_{3}\mathrm{COO}^{-}$ |
| --- | --- | --- | --- | --- | --- | --- | --- | --- | --- |
| $\Lambda_{0}$ | 6.2 | 7.4 | 5.0 | 35.0 | 7.2 | 7.6 | 16.0 | 19.9 | 4.1 |

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.

List-I
(P) Titrate: KCl; Titrant: $\mathrm{AgNO}_{3}$
(Q) Titrate: $\mathrm{AgNO}_{3}$; Titrant: KCl
(R) Titrate: NaOH; Titrant: HCl
(S) Titrate: NaOH; Titrant: $\mathrm{CH}_{3}\mathrm{COOH}$

List-II
(1) (see graph)
(2) (see graph)
(3) (see graph)
(4) (see graph)
(5) (see graph)

Accepted Answer

(C) $\mathrm{P} \rightarrow 3$, $\mathrm{Q} \rightarrow 4$, $\mathrm{R} \rightarrow 2$, $\mathrm{~S} \rightarrow 5$

Answer

(A) $\mathrm{P} \rightarrow 4$, $\mathrm{Q} \rightarrow 3$, $\mathrm{R} \rightarrow 2$, $\mathrm{~S} \rightarrow 5$

Answer

(B) $\mathrm{P} \rightarrow 2$, $\mathrm{Q} \rightarrow 4$, $\mathrm{R} \rightarrow 3$, $\mathrm{~S} \rightarrow 1$

Answer

(D) $\mathrm{P} \rightarrow 4$, $\mathrm{Q} \rightarrow 3$, $\mathrm{R} \rightarrow 2$, $\mathrm{~S} \rightarrow 1$

JEE Advanced · 2024 · 26 May 2024 · Paper 1 · Redox Reactions and Electrochemistry

Solution

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